In which reaction will an increase in the volume of the container favor the formation of products?

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)

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H_{2} O (g) + I_{2} (g) ⇌ 2 H I (g)

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4 N H_{3} (g) + 5 O_{2} (g) ⇌ 4 N O (g) + 6 H_{2} O (l)

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3 O_{2} (g) ⇌ 2 O_{3} (g)

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Solution

The correct option is A $C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)$
$V \propto n$ (gaseous moles)
$Δ n > 0 \to V > 0$ in option $(A)$ .

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Similar questions

Q. Write the expression for the equillibrium constant

(K_{c})

for the following reactions.
(i)

H_{2} (g) + I_{2} (g) ⇋ 2 H I (g)

(ii)

4 {N H}_{3} (g) + 5 O_{2} (g) ⇋ 4 N O (g) + 6 H_{2} O (g)

Q. For the reaction,

C (s) + H_{2} O (g) ⇌ H_{2} (g) + C O (g)

, by increasing pressure following equilibrium :

Q. Predict the effect upon the following reaction equilibria of increased pressure.

(1) H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g) (2) C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g) (3) C (s) + H_{2} O (g) ⇌ H_{2} (g) + C O (g)

C_{(s)} + H_{2} O_{(g)} \to C O (g) + H_{2} (g)

The pressure on the system is increased in the above reaction then:

Calculate the equilibrium constant ( $K_{p}$ ) for the reaction, $C (s) + C O_{2} (g) ⇌ 2 C O (g)$ , at $1300 K$ from the following data:
$C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g); K_{p} (1300 K) = 3.9 a t m$

$H_{2} (g) + C O_{2} (g) ⇌ C O (g) + H_{2} O (g); K_{p} (1300 K) = 0.623 a t m$

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In which reaction will an increase in the volume of the container favor the formation of products?

The correct option is A C(s)+H2O(g)⇌CO(g)+H2(g)V∝n (gaseous moles)Δn>0→V>0 in option (A).

The correct option is A $C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)$
$V \propto n$ (gaseous moles)
$Δ n > 0 \to V > 0$ in option $(A)$ .