Nitrogen gas (N₂) reacts with hydrogen gas (H₂) to form ammonia (NH₃). At 200°C in a closed container, 1.0 atm of nitrogen gas is mixed with 2.1 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

To solve this problem, we can use the equilibrium constant expression for the reaction:
Kc = [NH3]/[N2][H2]
At equilibrium, let x be the amount (in atm) of ammonia formed. Then the partial pressures of nitrogen and hydrogen will be (1.0 - x) atm and (2.1 - x) atm, respectively. We can set up an equation for Kc using these values:
Kc = x/[(1.0 - x)(2.1 - x)]
We know that the total pressure at equilibrium is 2.1 atm, so we can use this to solve for x:
(1.0 - x) + (2.1 - x) + x = 2.1
3.1 - x = 2.1
x = 1.0
Now we can substitute x = 1.0 back into the equation for partial pressure of hydrogen:
(2.1 - x) = (2.1 - 1.0) atm = 1.1 atm
Therefore, the partial pressure of hydrogen gas at equilibrium is 1.1 atm, which corresponds to choice D.

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

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