Question on: SS2 Chemistry - Chemical Equilibrium
The equilibrium constant Kp for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) is 0.034 at a certain temperature. If the partial pressure of NOCl is 0.25 atm, calculate the partial pressures of NO and Cl2 at equilibrium.
To calculate the partial pressures of NO and Cl2 at equilibrium, we use the equilibrium constant expression in terms of partial pressures, Kp.
Kp = (P(NO)2 x P(Cl2)) / (P(NOCl)2)
Given that Kp = 0.034 and P(NOCl) = 0.25 atm, we can rearrange the equation to solve for the partial pressures of NO and Cl2:
P(NO)2 x P(Cl2) = Kp x P(NOCl)2
P(NO)^2 x P(Cl2) = 0.034 x (0.25)2
P(NO)2 x P(Cl2) = 0.034 x 0.0625
P(NO)2 x P(Cl2) ≈ 0.002125
Taking the square root of both sides, we have:
P(NO) x P(Cl2) ≈ √(0.002125)
Since the partial pressures of NO and Cl2 are equal at equilibrium, we can assign them the same value, which we'll denote as x:
x2 ≈ √(0.002125)
x ≈ √(√0.002125)
x ≈ 0.0918
Therefore, the partial pressures of NO and Cl2 at equilibrium are approximately 0.0918 atm.
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