For the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g) + Heat; the equilibrium co

1.	For the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g) + Heat; the equilibrium constant K = 0.50 at 673K(a) Write the expression for Kc and Kp.(b) What will be the equilibrium constant value for the reverse reaction at 673K?(c) What is the effect if increasing temperature on the yield of NH3?(d) What is the effect adding N2(g) and H2(g) on the yield of NH3?(e) What is the effect of increasing pressure on the yield of NH3?
Answer» (a) K_c = \(\frac{[NH_3]^2}{[N_2][H_2]^3}\) And K_p = \(\frac{[P_{NH_3}]^2}{P_{N_2}\times(P_{H_2})^3}\) (b) K_eq. (For reverse reaction) = \(\frac{1}{K}\) = \(\frac{1}{0.50}\) = 2 (c) As this is an exothermic reaction, on increasing the temperature, the reaction will proceed in reverse direction. This results in decrease in concentration of NH₃. (d) On increasing the concentration of N₂(g) and H₂(g), the yield of NH₃ will increase. (e) On increasing the pressure, the reaction will proceed in forward reaction in which number of moles of gas or pressure decreases.

For the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g) + Heat; the equilibrium constant K = 0.50 at 673K(a) Write the expression for Kc and Kp.(b) What will be the equilibrium constant value for the reverse reaction at 673K?(c) What is the effect if increasing temperature on the yield of NH3?(d) What is the effect adding N2(g) and H2(g) on the yield of NH3?(e) What is the effect of increasing pressure on the yield of NH3?

Answer»

(a) K_c = \(\frac{[NH_3]^2}{[N_2][H_2]^3}\)

And K_p = \(\frac{[P_{NH_3}]^2}{P_{N_2}\times(P_{H_2})^3}\)

(b) K_eq. (For reverse reaction) = \(\frac{1}{K}\) = \(\frac{1}{0.50}\) = 2

(c) As this is an exothermic reaction, on increasing the temperature, the reaction will proceed in reverse direction. This results in decrease in concentration of NH₃.

(d) On increasing the concentration of N₂(g) and H₂(g), the yield of NH₃ will increase.

(e) On increasing the pressure, the reaction will proceed in forward reaction in which number of moles of gas or pressure decreases.

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