JEE Main Chemistry question

For the Haber's process for formation of NH₃ at 298 K: N₂+3H₂⇌2NH₃; ΔH=−460 kJ. Which of the following is correct?

(A)The condition for equilibrium is ₂+₂=₃, where G is Gibbs energy per mole of gaseous species measured at that partial pressureCorrect
(B)On addition of N₂, the equilibrium will shift to forward direction because according to II law of thermodynamics the entropy must decrease in the direction of spontaneous reaction
(C)The catalyst will increase the rate of forward reaction by 2 times and that of backward reaction by 1.5 times
(D)None of the above

Answer: (A)

Solution

(A) correctly states the chemical-potential equality condition for equilibrium.

Question ID VK-136053