Which of the following equilibria will shift | vedclass

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(C) According to Le Chatelier's principle,increasing the temperature favors the endothermic direction of a reaction.
$A$. $CO_{(g)} + H_2O_{(g)}

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,increasing the temperature favors the endothermic direction of a reaction.
$A$. $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ is exothermic $(\Delta H < 0)$.
$B$. $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is exothermic $(\Delta H < 0)$.
$C$. $H_2O_{(g)} \rightleftharpoons H_{2(g)} + \frac{1}{2}O_{2(g)}$ is endothermic $(\Delta H > 0)$.
$D$. $4HCl_{(g)} + O_{2(g)} \rightleftharpoons 2H_2O_{(g)} + 2Cl_{2(g)}$ is exothermic $(\Delta H < 0)$.
Therefore,increasing the temperature will shift the equilibrium to the right for reaction $C$.

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

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