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20,132,801 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 76.28 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 76.28 g therefore contains n = m / M = 76.28 / 44.01 = 1.733 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,802 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2O from mass 35.44 g | The molar mass of H2O is 18.02 g/mol. A sample of mass 35.44 g therefore contains n = m / M = 35.44 / 18.02 = 1.967 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,803 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 91.68 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 91.68 g therefore contains n = m / M = 91.68 / 159.7 = 0.5741 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,804 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CaCO3 from mass 58.09 g | The molar mass of CaCO3 is 100.1 g/mol. A sample of mass 58.09 g therefore contains n = m / M = 58.09 / 100.1 = 0.5804 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,805 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of C6H12O6 from mass 63.37 g | The molar mass of C6H12O6 is 180.2 g/mol. A sample of mass 63.37 g therefore contains n = m / M = 63.37 / 180.2 = 0.3517 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,806 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 55.84 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 55.84 g therefore contains n = m / M = 55.84 / 58.44 = 0.9555 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,807 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 12.37 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 12.37 g therefore contains n = m / M = 12.37 / 17.03 = 0.7264 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,808 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 8.811 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 8.811 g therefore contains n = m / M = 8.811 / 159.7 = 0.05518 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,809 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 88.71 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 88.71 g therefore contains n = m / M = 88.71 / 44.01 = 2.016 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,810 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 43.28 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 43.28 g therefore contains n = m / M = 43.28 / 159.7 = 0.271 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,811 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 25.14 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 25.14 g therefore contains n = m / M = 25.14 / 17.03 = 1.476 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,812 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 90.71 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 90.71 g therefore contains n = m / M = 90.71 / 16.04 = 5.654 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,813 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CaCO3 from mass 55.04 g | The molar mass of CaCO3 is 100.1 g/mol. A sample of mass 55.04 g therefore contains n = m / M = 55.04 / 100.1 = 0.5499 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,814 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 61.06 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 61.06 g therefore contains n = m / M = 61.06 / 58.44 = 1.045 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,815 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 25.82 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 25.82 g therefore contains n = m / M = 25.82 / 16.04 = 1.609 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,816 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 21.18 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 21.18 g therefore contains n = m / M = 21.18 / 58.44 = 0.3624 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,817 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 29.62 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 29.62 g therefore contains n = m / M = 29.62 / 98.07 = 0.302 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,818 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 59.03 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 59.03 g therefore contains n = m / M = 59.03 / 159.7 = 0.3696 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,819 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 61.92 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 61.92 g therefore contains n = m / M = 61.92 / 58.44 = 1.06 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,820 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 85.06 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 85.06 g therefore contains n = m / M = 85.06 / 159.7 = 0.5327 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,821 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 90.85 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 90.85 g therefore contains n = m / M = 90.85 / 44.01 = 2.064 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,822 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 94.07 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 94.07 g therefore contains n = m / M = 94.07 / 16.04 = 5.863 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,823 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 75.15 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 75.15 g therefore contains n = m / M = 75.15 / 98.07 = 0.7662 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,824 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CaCO3 from mass 66.7 g | The molar mass of CaCO3 is 100.1 g/mol. A sample of mass 66.7 g therefore contains n = m / M = 66.7 / 100.1 = 0.6664 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,825 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 6.782 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 6.782 g therefore contains n = m / M = 6.782 / 98.07 = 0.06915 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,826 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 8.91 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 8.91 g therefore contains n = m / M = 8.91 / 58.44 = 0.1525 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,827 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 10.6 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 10.6 g therefore contains n = m / M = 10.6 / 58.44 = 0.1814 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,828 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 59.94 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 59.94 g therefore contains n = m / M = 59.94 / 16.04 = 3.736 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,829 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 52.49 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 52.49 g therefore contains n = m / M = 52.49 / 58.44 = 0.8981 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,830 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 66.48 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 66.48 g therefore contains n = m / M = 66.48 / 16.04 = 4.144 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,831 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2O from mass 85.74 g | The molar mass of H2O is 18.02 g/mol. A sample of mass 85.74 g therefore contains n = m / M = 85.74 / 18.02 = 4.759 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,832 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 54.05 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 54.05 g therefore contains n = m / M = 54.05 / 44.01 = 1.228 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,833 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 45.78 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 45.78 g therefore contains n = m / M = 45.78 / 98.07 = 0.4668 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,834 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 81.65 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 81.65 g therefore contains n = m / M = 81.65 / 44.01 = 1.855 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,835 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 49.57 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 49.57 g therefore contains n = m / M = 49.57 / 17.03 = 2.911 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,836 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 59.4 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 59.4 g therefore contains n = m / M = 59.4 / 17.03 = 3.488 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,837 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 20.41 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 20.41 g therefore contains n = m / M = 20.41 / 159.7 = 0.1278 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,838 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 12.3 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 12.3 g therefore contains n = m / M = 12.3 / 98.07 = 0.1255 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,839 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2O from mass 1.415 g | The molar mass of H2O is 18.02 g/mol. A sample of mass 1.415 g therefore contains n = m / M = 1.415 / 18.02 = 0.07855 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,840 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2O from mass 33.04 g | The molar mass of H2O is 18.02 g/mol. A sample of mass 33.04 g therefore contains n = m / M = 33.04 / 18.02 = 1.834 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,841 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 46.92 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 46.92 g therefore contains n = m / M = 46.92 / 58.44 = 0.8029 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,842 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CH4 from mass 22.34 g | The molar mass of CH4 is 16.04 g/mol. A sample of mass 22.34 g therefore contains n = m / M = 22.34 / 16.04 = 1.393 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,843 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2O from mass 24.84 g | The molar mass of H2O is 18.02 g/mol. A sample of mass 24.84 g therefore contains n = m / M = 24.84 / 18.02 = 1.379 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,844 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 8.058 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 8.058 g therefore contains n = m / M = 8.058 / 44.01 = 0.1831 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,845 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 29.87 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 29.87 g therefore contains n = m / M = 29.87 / 44.01 = 0.6787 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,846 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 54.36 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 54.36 g therefore contains n = m / M = 54.36 / 17.03 = 3.192 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,847 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of H2SO4 from mass 65.61 g | The molar mass of H2SO4 is 98.07 g/mol. A sample of mass 65.61 g therefore contains n = m / M = 65.61 / 98.07 = 0.669 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,848 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of C6H12O6 from mass 86.76 g | The molar mass of C6H12O6 is 180.2 g/mol. A sample of mass 86.76 g therefore contains n = m / M = 86.76 / 180.2 = 0.4816 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,849 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of Fe2O3 from mass 87.17 g | The molar mass of Fe2O3 is 159.7 g/mol. A sample of mass 87.17 g therefore contains n = m / M = 87.17 / 159.7 = 0.5459 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,850 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 1.198 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 1.198 g therefore contains n = m / M = 1.198 / 17.03 = 0.07032 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,851 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NH3 from mass 86.29 g | The molar mass of NH3 is 17.03 g/mol. A sample of mass 86.29 g therefore contains n = m / M = 86.29 / 17.03 = 5.067 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,852 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 42.35 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 42.35 g therefore contains n = m / M = 42.35 / 58.44 = 0.7247 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,853 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of NaCl from mass 35.36 g | The molar mass of NaCl is 58.44 g/mol. A sample of mass 35.36 g therefore contains n = m / M = 35.36 / 58.44 = 0.6051 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,854 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 72.79 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 72.79 g therefore contains n = m / M = 72.79 / 44.01 = 1.654 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,855 | chemistry | stoichiometry | mole_concept | 3 | worked_example | Moles of CO2 from mass 67.51 g | The molar mass of CO2 is 44.01 g/mol. A sample of mass 67.51 g therefore contains n = m / M = 67.51 / 44.01 = 1.534 mol. The mole is the SI unit for amount of substance and links macroscopic mass to number of entities via Avogadro's constant. | n = m / M | atomic masses; chemical formulas | Convert between mass and moles for a pure compound. |
20,132,856 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.509 mol, V=32.74 L, T=492.7 K | For an ideal gas, P V = n R T. With n = 2.509 mol, V = 32.74 L, T = 492.7 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.098 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,857 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.5207 mol, V=24.1 L, T=565 K | For an ideal gas, P V = n R T. With n = 0.5207 mol, V = 24.1 L, T = 565 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.002 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,858 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.96 mol, V=10.61 L, T=506.7 K | For an ideal gas, P V = n R T. With n = 2.96 mol, V = 10.61 L, T = 506.7 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 11.6 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,859 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.179 mol, V=27.42 L, T=535.6 K | For an ideal gas, P V = n R T. With n = 1.179 mol, V = 27.42 L, T = 535.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.889 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,860 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.236 mol, V=40.42 L, T=496.6 K | For an ideal gas, P V = n R T. With n = 3.236 mol, V = 40.42 L, T = 496.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.263 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,861 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.624 mol, V=44.01 L, T=595.3 K | For an ideal gas, P V = n R T. With n = 0.624 mol, V = 44.01 L, T = 595.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.6927 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,862 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.6202 mol, V=22.39 L, T=435.7 K | For an ideal gas, P V = n R T. With n = 0.6202 mol, V = 22.39 L, T = 435.7 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.9902 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,863 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.921 mol, V=13.11 L, T=230.7 K | For an ideal gas, P V = n R T. With n = 1.921 mol, V = 13.11 L, T = 230.7 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 2.774 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,864 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.129 mol, V=7.294 L, T=209.4 K | For an ideal gas, P V = n R T. With n = 1.129 mol, V = 7.294 L, T = 209.4 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 2.659 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,865 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.115 mol, V=40.77 L, T=559.2 K | For an ideal gas, P V = n R T. With n = 1.115 mol, V = 40.77 L, T = 559.2 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.254 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,866 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.499 mol, V=18.68 L, T=356.3 K | For an ideal gas, P V = n R T. With n = 1.499 mol, V = 18.68 L, T = 356.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 2.346 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,867 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.141 mol, V=11.77 L, T=504.6 K | For an ideal gas, P V = n R T. With n = 4.141 mol, V = 11.77 L, T = 504.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 14.57 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,868 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.045 mol, V=18.34 L, T=208.1 K | For an ideal gas, P V = n R T. With n = 4.045 mol, V = 18.34 L, T = 208.1 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.766 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,869 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.768 mol, V=25.21 L, T=262.3 K | For an ideal gas, P V = n R T. With n = 3.768 mol, V = 25.21 L, T = 262.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.218 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,870 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.967 mol, V=0.7594 L, T=242.6 K | For an ideal gas, P V = n R T. With n = 4.967 mol, V = 0.7594 L, T = 242.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 130.2 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,871 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.4069 mol, V=38.6 L, T=418.5 K | For an ideal gas, P V = n R T. With n = 0.4069 mol, V = 38.6 L, T = 418.5 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.362 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,872 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.979 mol, V=14.66 L, T=546.3 K | For an ideal gas, P V = n R T. With n = 2.979 mol, V = 14.66 L, T = 546.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 9.107 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,873 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.2622 mol, V=16.5 L, T=455.4 K | For an ideal gas, P V = n R T. With n = 0.2622 mol, V = 16.5 L, T = 455.4 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.5938 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,874 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.916 mol, V=5.248 L, T=475.3 K | For an ideal gas, P V = n R T. With n = 2.916 mol, V = 5.248 L, T = 475.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 21.67 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,875 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.309 mol, V=26.83 L, T=455.2 K | For an ideal gas, P V = n R T. With n = 3.309 mol, V = 26.83 L, T = 455.2 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 4.606 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,876 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.9388 mol, V=29.59 L, T=298.5 K | For an ideal gas, P V = n R T. With n = 0.9388 mol, V = 29.59 L, T = 298.5 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.7772 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,877 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.064 mol, V=33.28 L, T=401.1 K | For an ideal gas, P V = n R T. With n = 3.064 mol, V = 33.28 L, T = 401.1 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.029 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,878 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.02 mol, V=23.5 L, T=289.9 K | For an ideal gas, P V = n R T. With n = 4.02 mol, V = 23.5 L, T = 289.9 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 4.068 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,879 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.487 mol, V=22.25 L, T=221.8 K | For an ideal gas, P V = n R T. With n = 4.487 mol, V = 22.25 L, T = 221.8 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 3.67 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,880 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.048 mol, V=2.036 L, T=505.4 K | For an ideal gas, P V = n R T. With n = 3.048 mol, V = 2.036 L, T = 505.4 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 62.09 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,881 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.5651 mol, V=33.38 L, T=285.3 K | For an ideal gas, P V = n R T. With n = 0.5651 mol, V = 33.38 L, T = 285.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.3963 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,882 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.555 mol, V=19.13 L, T=598.6 K | For an ideal gas, P V = n R T. With n = 3.555 mol, V = 19.13 L, T = 598.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 9.127 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,883 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.469 mol, V=18.24 L, T=520 K | For an ideal gas, P V = n R T. With n = 3.469 mol, V = 18.24 L, T = 520 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 8.115 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,884 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.04065 mol, V=12.2 L, T=465.4 K | For an ideal gas, P V = n R T. With n = 0.04065 mol, V = 12.2 L, T = 465.4 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.1272 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,885 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.594 mol, V=18.23 L, T=463.3 K | For an ideal gas, P V = n R T. With n = 2.594 mol, V = 18.23 L, T = 463.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 5.411 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,886 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.098 mol, V=32.63 L, T=221.6 K | For an ideal gas, P V = n R T. With n = 3.098 mol, V = 32.63 L, T = 221.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.726 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,887 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.771 mol, V=39.73 L, T=250.2 K | For an ideal gas, P V = n R T. With n = 1.771 mol, V = 39.73 L, T = 250.2 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.9154 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,888 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.166 mol, V=18.37 L, T=359.1 K | For an ideal gas, P V = n R T. With n = 1.166 mol, V = 18.37 L, T = 359.1 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.871 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,889 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.641 mol, V=33.25 L, T=387.2 K | For an ideal gas, P V = n R T. With n = 2.641 mol, V = 33.25 L, T = 387.2 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 2.524 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,890 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.862 mol, V=25.37 L, T=588.6 K | For an ideal gas, P V = n R T. With n = 2.862 mol, V = 25.37 L, T = 588.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 5.448 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,891 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.548 mol, V=30.96 L, T=391.6 K | For an ideal gas, P V = n R T. With n = 0.548 mol, V = 30.96 L, T = 391.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.5686 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,892 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.135 mol, V=31.26 L, T=416.2 K | For an ideal gas, P V = n R T. With n = 4.135 mol, V = 31.26 L, T = 416.2 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 4.517 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,893 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.211 mol, V=18.75 L, T=581.8 K | For an ideal gas, P V = n R T. With n = 3.211 mol, V = 18.75 L, T = 581.8 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 8.174 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,894 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=3.588 mol, V=2.764 L, T=246.6 K | For an ideal gas, P V = n R T. With n = 3.588 mol, V = 2.764 L, T = 246.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 26.27 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,895 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=1.811 mol, V=28.3 L, T=273.6 K | For an ideal gas, P V = n R T. With n = 1.811 mol, V = 28.3 L, T = 273.6 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.436 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,896 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=2.281 mol, V=22.6 L, T=280.3 K | For an ideal gas, P V = n R T. With n = 2.281 mol, V = 22.6 L, T = 280.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 2.321 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,897 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.2368 mol, V=20.81 L, T=339.3 K | For an ideal gas, P V = n R T. With n = 0.2368 mol, V = 20.81 L, T = 339.3 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 0.3168 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,898 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=4.029 mol, V=6.293 L, T=563.4 K | For an ideal gas, P V = n R T. With n = 4.029 mol, V = 6.293 L, T = 563.4 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 29.6 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,899 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.4474 mol, V=16.64 L, T=577 K | For an ideal gas, P V = n R T. With n = 0.4474 mol, V = 16.64 L, T = 577 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 1.273 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
20,132,900 | chemistry | gases | ideal_gas_law | 4 | worked_example | Ideal-gas pressure for n=0.6627 mol, V=4.647 L, T=442.5 K | For an ideal gas, P V = n R T. With n = 0.6627 mol, V = 4.647 L, T = 442.5 K and R = 0.082057 L·atm·mol⁻¹·K⁻¹, the pressure is P = n R T / V = 5.179 atm. Real gases approach ideal behavior at low pressure and high temperature relative to their critical points. | P V = n R T | mole_concept | Apply the ideal-gas law to compute pressure, volume, or temperature. |
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