Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?

(i) $P C l_{5} (g) \leftrightarrow P C l_{3} (g) + C l_{2} (g)$

(ii) $C a O (s) + C O_{2} (g) \leftrightarrow C a C O_{3} (s)$

(iii) $3 F e (s) + 4 H_{2} O (g) \leftrightarrow F e_{3} O_{4} (s) + 4 H_{2} (g)$

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Solution

(i) The number of moles of reaction products will increase. According to Le Chatelier's principle, if pressure is decreased, then the equilibrium shifts in the direction in which the number of moles of gases is rnore. In the given reaction, the number of moles of gaseous products is more than that of gaseous reactan.. Thus, the reaction will proceed in the forward direction. As a result, the nurnber of rnoles of reaction products will increase.

(ii) The number of rnoles of reaction products will decrease.

(iii) The number of moles of reaction products remains the same.

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Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?

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Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?

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(b)

(c)

Q. Does the number of moles of reaction products increase, decrease or remain same when each of the following equiibria is subjected to a decrease in pressure bp increasing the volume?
i)

P C l_{5} ⇌ P C l_{3} (g) + C l_{2} (g)

ii)

C a O (s) + C O_{2} (g) ⇌ C a C O_{3} (s)

iii)

3 F e (s) + 4 H_{2} O (g) ⇌ F e_{3} O_{4} (s) + 4 H_{2} (g)

Which of the following reactions will get affected by increasing the pressure?
Also, mention whether change will cause the reaction to go into forward or backward direction.
(i) $C O C l_{2} (g) \leftrightarrow C O (g) + C l_{2} (g)$
(ii) $C H_{4} (g) + 2 S_{2} (g) \leftrightarrow C S_{2} (g) + 2 H_{2} S (g)$
(iii) $C O_{2} (g) + C (s) \leftrightarrow 2 C O (g)$
(iv) $2 H_{2} (g) + C O (g) \leftrightarrow C H_{3} O H (g)$
(v) $C a C O_{3} (s) \leftrightarrow C a O (s) + C O_{2} (g)$
(vi) $4 N H_{3} (g) + 5 O_{2} (g) \leftrightarrow 4 N O (g) + 6 H_{2} O (g)$