Question

At constant pressure, addition of helium to the reaction system :

N₂ (g) + 3H₂ (g) $\rightleftarrows$ 2NH₃ (g)

• A. Favours the formation of ammonia
• B. Reduces the formation of ammonia
• C. Does not affect the position of equilibrium
• D. Reduces the dissociation of ammonia.

Answer 1

Answer: (B)

Reduces the formation of ammonia

Answer 2

K_p = $\frac { \mathrm { n } _ { \mathrm { NH } _ { 3 } } ^ { 2 } } { \mathrm { n } _ { \mathrm { N } _ { 2 } } \times \mathrm { n } _ { \mathrm { H } _ { 2 } } ^ { 3 } }$×

At constant pressure, with the introduction inert gas Sn increases. Since Dn = –2, therefore on increasing Sn increases, but K_p remain constant, hence no. of

moles of N₂ (g) & H₂ (g) are increased and backward reaction is favoured.