Advertisements
Advertisements
Question
112 cm3 of H2S(g) is mixed with 120 cm3 of Cl2(g) at STP to produce HCl(g) and sulphur(s). Write a balanced equation for this reaction and calculate
- the volume of gaseous product formed.
- composition of the resulting mixture.
Advertisements
Solution
\[\ce{H2S + Cl2 -> 2HCl + S}\]
(i)
At STP,
1 mole gas occupies = 22.4 L.
1 mole H2S gas produces = 2 moles HCl gas,
∴ 22.4 L H2S gas produces
= 22.4 × 2
= 44.8 L HCl gas.
Hence, 112 cm3 H2S gas will produce
= 112 × 2
= 224 cm3 HCl gas.
Hence, 224 cm3 HCl gas is produced.
(ii)
1 mole H2S gas consumes = 1 mole Cl2 gas.
Hence, 22.4 L H2S gas consumes = 22.4 L Cl2 gas at STP.
∴ 112 cm3 H2S gas consumes = 112 cm3 Cl2 gas.
120 cm3 − 112 cm3 = 8 cm3 Cl2 gas remains unreacted.
Hence, the composition of the resulting mixture is 224 cm3 HCl gas + 8 cm3 Cl2 gas.
RELATED QUESTIONS
State Gay-Lussac's law of combining volumes.
How does Avogadro's law explain Gay - lussac's law of combining volumes?
Water can split into hydrogen and oxygen under suitable conditions. The equations representing the change is: 2H2O(I) → 2H2 (g) + O2(g)
If a given experiment results in 2500cm3 of hydrogen being produced, what volume of oxygen is liberated at the same time under the same conditions of temperature and pressure?
The reaction 4N2O + CH4 → CO2 + 2H2O + 4N2 takes place in the gaseous state. If the volumes of all the gases are measured at the same temperature, and pressure, calculate the volume of dinitrogen oxide (N2O), required to give 150cm3 of steam.
Calcium carbide is used for the artificial ripening of fruits. Actually the fruit ripens because of the heat evolved while calcium carbide reacts with the moisture. During this reaction calcium hydroxide and acetylene gas are formed. If 200 cm3 of acetylene is formed from a certain mass of calcium carbide, find the volume of oxygen required and carbon dioxide formed during the complete combustion. The combustion reaction can be represented as below.
\[\ce{2C2H2_{(g)} + 5O2_{(g)}-> 4CO2_{(g)} + 2H2O_{(g)}}\]
24 cc Marsh gas (CH4) was mixed with 106 cc oxygen and then exploded. On cooling the volume of the mixture became 82 cc, of which, 58 cc was unchanged oxygen. Which law does this experiment support? Explain with calculations.
1250 cc of oxygen was burnt with 300cc of ethane [C2H6]. Calculate the volume of carbon dioxide formed:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
A mixture of hydrogen and chlorine occupying 36 cm3 was exploded. On shaking it with water, 4 cm3 of hydrogen was left behind. Find the composition of the mixture.
LPG has 60% propane and 40% butane: 10 litres of this mixture is burnt. Calculate the volume of carbon dioxide added to atmosphere.
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
\[\ce{2C4H10 + 13O2 → 8CO2 + 10H2O}\]
200 cm3 of CO2 is collected at STP when a mixture of acetylene and oxygen is ignited. Calculate the volume of acetylene and oxygen at STP. in original mixture.
\[\ce{2C2H2_{(g)} + 5O2_{(g)} → 4CO2_{(g)} + 2H2O_{(g)}}\]
