What is the value of the equilibrium constant for the Haber process at 298K if t

Question

What is the value of the equilibrium constant for the Haber process at 298K if the equilibrium concentrations are as follows: (H_2] = 0.0368M, [N_2] = 0.0512M. and [NH_3] = 1.33M. Methyl red is an indicator that changes between red and yellow. In solution methyl red (HMR) dissociates as follows: If acid is added to the solution which way do you expect the equilibrium to shift? What color would the indicator be? Explain your conclusion: If base is added to the solution which way do you expect the equilibrium to shift? What color would the indicator be? Explain your conclusion:

Explanation / Answer

We know that,

Haber's process is used for the manufacture of ammonia. Reaction involved is as follows:

N2 (g) + 3H2 (g) ----> 2NH3 (g)

Equilibrium constant, Kc = [NH3]2 / [N2] [H2]3

Kc = 6.936 x 105

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