Which of the following equilibria will shift | vedclass

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Question

(C) According to Le Chatelier's principle,an increase in temperature favors the endothermic direction of a reaction.
Reaction $(a)$ is the water-

Vedclass · Accepted Answer

$H_2O_{(g)} \rightleftharpoons H_{2_{(g)}} + \frac{1}{2}O_{2_{(g)}}$

Vedclass · Answer

(C) According to Le Chatelier's principle,an increase in temperature favors the endothermic direction of a reaction.
Reaction $(a)$ is the water-gas shift reaction,which is exothermic $(\Delta H < 0)$.
Reaction $(b)$ is the contact process step,which is exothermic $(\Delta H < 0)$.
Reaction $(c)$ represents the thermal decomposition of water,which is highly endothermic $(\Delta H > 0)$.
Reaction $(d)$ is the Deacon process,which is exothermic $(\Delta H < 0)$.
Therefore,only reaction $(c)$ will shift to the right side upon increasing the temperature.

Which of the following equilibria will shift to the right side on increasing the temperature?

Similar Questions

In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

What happens when pressure is increased on the equilibrium system $Ice \rightleftharpoons Water$?

Le Chatelier's principle is applicable to:

Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.
Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.

Which of the following information can be obtained on the basis of Le Chatelier's principle?

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