The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures, 400° C and 500° C. Which of the following graph correctly represent the process?

Question

The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures, 400° C and 500° C. Which of the following graph correctly represent the process? (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

N 2( g )+3 H 2( g ) leftharpoons 2 NH 3( g ) ; Δ H < 0 By Le Chatelier principle, higher pressure and lower temperature favour the forward reaction, i.e., higher % of NH 3.

Q. The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures, $40 0^{\circ} C$ and $50 0^{\circ} C$ . Which of the following graph correctly represent the process?

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); Δ H < 0$

By Le Chatelier principle, higher pressure and lower temperature favour the forward reaction, i.e., higher $%$ of $N H_{3}$ .

Q. The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures, 400∘C and 500∘C. Which of the following graph correctly represent the process?

N2​(g)+3H2​(g)⇌2NH3​(g);ΔH<0 By Le Chatelier principle, higher pressure and lower temperature favour the forward reaction, i.e., higher % of NH3​.

Q. The percentage of ammonia obtainable, if equilibrium were to be established during the Haber process, is plotted against the operating pressure for two temperatures, $40 0^{\circ} C$ and $50 0^{\circ} C$ . Which of the following graph correctly represent the process?

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g); Δ H < 0$

By Le Chatelier principle, higher pressure and lower temperature favour the forward reaction, i.e., higher $%$ of $N H_{3}$ .