If 6 litres of hydrogen and 4 litres of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.
Stoichiometry
234 Likes

Question

If 6 litres of hydrogen and 4 litres of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.

KnowledgeBoat · Accepted Answer

[By Lussac's law] To calculate the amount of hydrogen used: Remaining hydrogen = 6 - 4 = 2 lit. To calculate the amount of HCl : Hence, after reaction 8 lit of HCl is formed which dissolves in water and 2 lit of hydrogen is left. 2 lits. of hydrogen is left.

Chemistry

If 6 litres of hydrogen and 4 litres of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.

Stoichiometry

Related Questions

What volume of oxygen is required to burn completely 90 dm³ of butane under similar conditions of temperature and pressure?
2C₄H₁₀ + 13O₂ ⟶ 8CO₂ + 10H₂O

What volume of ethyne gas at s.t.p. is required to produce 8.4 dm³ of carbon dioxide at s.t.p.?
2C₂H₂ + 5O₂ ⟶ 4CO₂ + 2H₂O
[H = 1, C = 12, O = 16]

The equation :
4NH₃ + 5O₂ ⟶ 4NO + 6H₂O,
represents the catalytic oxidation of ammonia. If 100 cm³ of ammonia is used calculate the volume of oxygen required to oxidize the ammonia completely.

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.

Chemistry

If 6 litres of hydrogen and 4 litres of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.

Stoichiometry

Related Questions

What volume of oxygen is required to burn completely 90 dm3 of butane under similar conditions of temperature and pressure?2C4H10 + 13O2 ⟶ 8CO2 + 10H2O

What volume of ethyne gas at s.t.p. is required to produce 8.4 dm3 of carbon dioxide at s.t.p.?2C2H2 + 5O2 ⟶ 4CO2 + 2H2O[H = 1, C = 12, O = 16]

The equation :4NH3 + 5O2 ⟶ 4NO + 6H2O,represents the catalytic oxidation of ammonia. If 100 cm3 of ammonia is used calculate the volume of oxygen required to oxidize the ammonia completely.

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.

What volume of oxygen is required to burn completely 90 dm³ of butane under similar conditions of temperature and pressure?
2C₄H₁₀ + 13O₂ ⟶ 8CO₂ + 10H₂O

What volume of ethyne gas at s.t.p. is required to produce 8.4 dm³ of carbon dioxide at s.t.p.?
2C₂H₂ + 5O₂ ⟶ 4CO₂ + 2H₂O
[H = 1, C = 12, O = 16]

The equation :
4NH₃ + 5O₂ ⟶ 4NO + 6H₂O,
represents the catalytic oxidation of ammonia. If 100 cm³ of ammonia is used calculate the volume of oxygen required to oxidize the ammonia completely.

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.