Nitrogen gas (N₂) reacts with hydrogen gas (H₂) to form ammonia (NH₃). At 200°C in a closed container, 1.2atm of nitrogen gas is mixed with 2.3 atm of hydrogen gas. At equilibrium, the total pressure is 2.1 atm. Calculate the partial pressure of hydrogen gas at equilibrium.

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:
N2 + 3H2→ 2NH3
At the beginning, the partial pressures of nitrogen gas and hydrogen gas are 1.2 atm and 2.3 atm, respectively. Let x be the change in pressure due to the formation of ammonia. Therefore,
Partial pressure of nitrogen gas at equilibrium  = 1.2 atm - x
Partial pressure of hydrogen gas at equilibrium = 2.3 atm - 3x
Partial pressure of ammonia gas at equilibrium  = 2x
According to the problem, the total pressure at equilibrium is 2.1 atm. Hence,
Partial pressure of nitrogen gas + Partial pressure of hydrogen gas + Partial pressure of ammonia gas = 2.1 atm
(1.2 - x) + (2.3 - 3x) + 2x = 2.1
Simplifying and solving for x gives x = 0.20 atm.
Therefore, the partial pressure of hydrogen gas at equilibrium is:
2.3 atm - 3x = 2.3 atm - 3(0.20 atm) = 1.7 atm.
Hence, the correct answer is D) 0.20 atm.

Nitrogen Gas (N2) Reacts with Hydrogen Gas (H2) to Form

Nitrogen Gas (N₂) Reacts with Hydrogen Gas (H₂) to Form