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.
APPEARS IN
RELATED QUESTIONS
Propane burns in air according to the following equation:
C3H8 + 5O2 → 3CO2 + 4H2O
What volume of propane is consumed on using 1000 cm3 of air, considering only 20% of air contains oxygen?
How does Avogadro's law explain Gay - lussac's law of combining volumes?
What volume of oxygen would be required for complete combustion of 100L of ethane according to the following equation?
2C2H6 + 7O2 → 4CO2 + 6H2O
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.
Propane burns in air according to the following equation:
\[\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}\]
What volume of propane is consumed on using 1000 cm3 of air, considering only 20% of air contains oxygen?
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.
What volume of propane is burnt for every 500 cm3 of air used in the reaction under the same conditions? (assuming oxygen is `1/5`th of air)
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
What volume of air (containing 20% O2 by volume) will be required to burn completely 10 cm3 of methane and acetylene?
\[\ce{CH4 + 2O2 → CO2 + 2H2O}\]
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
LPG has 60% propane and 40% butane: 10 litres of this mixture is burnt. Calculate the volume of carbon dioxide added to atmosphere.
\[\ce{C3H8 + 5O2 → 3CO2 + 4H2O}\]
\[\ce{2C4H10 + 13O2 → 8CO2 + 10H2O}\]
The reaction: \[\ce{4N2O + CH4 -> CO2 + 2H2O + 4N2}\] takes place in the gaseous state. If all volumes are measured at the same temperature and pressure, calculate the volume of dinitrogen oxide (N2O) required to give 150 cm3 of steam.
