Consider the water gas equilibrium reaction, C ( s )+ H 2 O ( g ) leftharpoons CO ( g )+ H 2( g ) Which of the following statements is true at equilibrium?

Question

Consider the water gas equilibrium reaction, C ( s )+ H 2 O ( g ) leftharpoons CO ( g )+ H 2( g ) Which of the following statements is true at equilibrium? (A) If the amount of C(s) is increased, less water would be formed (B) If the amount of C(s) is increased, more CO and H2 would be formed (C) If the pressure on the system is increased by halving the volume, more water would be formed (D) If the pressure on the system is increased by halving the volume, more CO and H2 would be formed

Tardigrade Admin · Accepted Answer

K = ([CO(g)][H2(g)]/[H2O(g)]) Concentration will increase, on halving the volume. There are two terms in numerator. So to keep K constant, concentration of [H2O] should increase much more.

Q. Consider the water gas equilibrium reaction, $C (s) + H_{2} O (g) ⇌ CO (g) + H_{2} (g)$ Which of the following statements is true at equilibrium?

If the amount of $C (s)$ is increased, less water would be formed

If the amount of $C (s)$ is increased, more $CO$ and $H_{2}$ would be formed

If the pressure on the system is increased by halving the volume, more water would be formed

If the pressure on the system is increased by halving the volume, more $CO$ and $H_{2}$ would be formed

$K = \frac{[ CO ( g ) ] [ H _{2} ( g ) ]}{[ H _{2} O ( g ) ]}$
Concentration will increase, on halving the volume. There are two terms in numerator. So to keep K constant, concentration of $[H_{2} O]$ should increase much more.

Q. Consider the water gas equilibrium reaction, C(s)+H2​O(g)⇌CO(g)+H2​(g) Which of the following statements is true at equilibrium?

If the amount of C(s) is increased, less water would be formed

If the amount of C(s) is increased, more CO and H2​ would be formed