If the synthesis of ammonia from Haber's process is carried out with exactly the same starting conditions (of partial pressure and temperature) but using D 2 (deuterium) in place of H 2. Then

Question

If the synthesis of ammonia from Haber's process is carried out with exactly the same starting conditions (of partial pressure and temperature) but using D 2 (deuterium) in place of H 2. Then (A) the equilibrium will be disturbed (B) the composition of reaction mixture will remain same at equilibrium. (C) Use of isotope in reaction will not produce ammonia. (D) At equilibrium rate of forward reaction will be greater than the rate of reverse reaction

Tardigrade Admin · Accepted Answer

The reaction mixtures starting either with H 2 or D 2 reach equilibrium with the same composition, except that D 2 and ND 3 are present instead of H 2 and NH 3.

Q. If the synthesis of ammonia from Haber's process is carried out with exactly the same starting conditions (of partial pressure and temperature) but using $D_{2}$ (deuterium) in place of $H_{2}$ . Then

the equilibrium will be disturbed

the composition of reaction mixture will remain same at equilibrium.

Use of isotope in reaction will not produce ammonia.

At equilibrium rate of forward reaction will be greater than the rate of reverse reaction

The reaction mixtures starting either with $H_{2}$ or $D_{2}$ reach equilibrium with the same composition, except that $D_{2}$ and $N D_{3}$ are present instead of $H_{2}$ and $N H_{3}$ .

Q. If the synthesis of ammonia from Haber's process is carried out with exactly the same starting conditions (of partial pressure and temperature) but using D2​ (deuterium) in place of H2​. Then