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Colourless and odorless gas produced
Solution formed turn blue litmus paper faint red
Red litmus paper remains red
Explanation
Carbon burns in air and faster in Oxygen with a blue nonsootynonsmoky flame forming Carbon IV oxide gas
Carbon burns in limited supply of air with a blue nonsootynonsmoky flame forming Carbon IV oxide gas
Carbon IV oxide gas dissolves in water to form weak acidic solution of Carbonic IV acid
Chemical Equation
Carbon Oxygen Carbon IV oxide
excess airoxygen
Cs O2 g CO2 g in excess air
Carbon Oxygen Carbon II oxide
limited airoxygen
2Cs O2 g 2CO g in limited air
Carbon IV oxide Water Carbonic IV acid
CO2 g H2O l H2CO3 aq very weak acid
II Burning Sulphur
Procedure
aUsing a deflagrating spoon place sulphur powder on a Bunsen flame
Observe
Place the products in a beaker containing about 3cm3 of water Test the solutionmixture using litmus papers
b Using a deflagrating spoon place sulphur powder on a Bunsen flame Slowly lower it into a gas jar containing Oxygen gas Observe
Place about 5cm3 of water Swirl Test the solutionmixture using litmus papers
Observations
Sulphur burns with a blue flame
Gas produced that has pungent choking smell
Solution formed turn blue litmus paper faint red
Red litmus paper remains red
Explanation
Sulphur burns in air and faster in Oxygen with a blue nonsootynonsmoky flame forming Sulphur IV oxide gas
Sulphur IV oxide gas dissolves in water to form weak acidic solution of Sulphuric IV acid
Chemical Equation
Sulphur Oxygen Sulphur IV oxide
Ss O2 g SO2 g in excess air
Sulphur IV oxide Water Sulphuric IV acid
SO2 g H2O l H2SO3 aq very weak acid
III Burning Phosphorus
Procedure
aRemove a small piece of phosphorus from water and using a deflagrating spoon with a lid cover places it on a Bunsen flame
Observe
Carefully put the burning phosphorus to cover gas jar containing about 3cm3 of water Test the solutionmixture using litmus papers
b Remove another small piece of phosphorus from water and using a deflagrating spoon with a lid cover place it on a Bunsen flame
Slowly lower it into a gas jar containing Oxygen gas with about 5 cm3 of water Observe
Swirl Test the solutionmixture using litmus papers
Observations
Phosphorus catches fire before heating on Bunsen flame
Dense white fumes of a gas produced that has pungent choking poisonous smell
Solution formed turn blue litmus paper faint red
Red litmus paper remains red
Explanation
Phosphorus is stored in water On exposure to air it instantaneously fumes then catch fire to burn in air and faster in Oxygen with a yellow flame producing dense white acidic fumes of Phosphorus V oxide gas
Phosphoric V oxide gas dissolves in water to form weak acidic solution of Phosphoric V acid
Chemical Equation
Phosphorus Oxygen Phosphorous V oxide
4Ps 5O2 g 2P2O5s
Phosphorous V oxide Water Phosphoric V acid
P2O5s 3H2O l 2H3PO4 aq very weak acid
e Reactivity seriescompetition for combined Oxygen
The reactivity series is a list of elementsmetals according to their affinity for oxygen
Some metals have higher affinity for Oxygen than others
A metalelement with higher affinity for oxygen is placed higheron top of the one less affinity
The complete reactivity series of metalselements
Metals compete for combined Oxygen A metalelement with higher affinity for oxygen removes Oxygen from a metal lower in the reactivity seriesless affinity for Oxygen
When a metalelement gainsacquire Oxygen the process is called Oxidation
When metalelement donatelose Oxygen the process is called Reduction
An elementmetalcompound that undergoes Oxidation is called Reducing agent
An elementmetalcompound that undergoes Reduction is called Oxidizing agent
A reaction in which both Oxidation and Reduction take place is called a Redox reaction
Redox reaction between Magnesium and copper II Oxide
Procedure
Place about 2g of copper II oxide in a crucible with a lid Place another 2g of Magnesium powder into the crucible Mix thoroughly
Cover the crucible with lid Heat strongly for five minutes
Allow the mixture to cool Open the lid Observe
Observation
Colour change from black to brown White solid power formed
Explanation
Magnesium is higher in the reactivity series than Copper It has therefore higher affinity for Oxygen than copper
When a mixture of copper II oxide and Magnesium is heated Magnesium reduces copper II oxide to brown copper metal and itself oxidized to Magnesium oxide Magnesium is the reducing agent because it undergoes oxidation process
Copper II oxide is the oxidizing agent because it undergoes redox reduction process
The mixture should be cooled before opening the lid to prevent hot brown copper from being reoxidized back to black copper II oxide
The reaction of Magnesium and Copper II oxide is a reaction
Chemical equation
1 Copper II oxide Magnesium Magnesium oxide Copper
black white ashsolid brown
CuOs Mgs MgOs Cus
Oxidizing Agent Reducing Agent
2 Zinc II oxide Magnesium Magnesium oxide Zinc
yellow when hot white ashsolid grey
ZnOs Mgs MgOs Zns
Oxidizing agent Reducing agent
3 Zinc II oxide Carbon Carbon IV oxide gas Zinc
yellow when hot colourless gas grey
ZnOs Cs CO2 g Zns
Oxidizing agent Reducing agent
The reactivity series is used during extraction of metals from their ore An ore is a rock containing mineral element which can be extracted for commercial purposes Most metallic ores occur naturally as
i oxides combined with Oxygen
ii sulphides combined with Sulphur
iii carbonates combined with carbon and Oxygen
Metallic ores that naturally occur as metallic sulphides are first roasted in air to form the corresponding oxide Sulphur IV oxide gas is produced eg
Copper I sulphide Oxygen Copper I Oxide Sulphur IV oxide