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(C) According to Le Chatelier's principle,an increase in temperature favors the endothermic reaction (where $\Delta H > 0$).$1$. The reaction $CO_{(g)

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

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(C) According to Le Chatelier's principle,an increase in temperature favors the endothermic reaction (where $\Delta H > 0$).$1$. The reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ is exothermic.$2$. The reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is exothermic.$3$. The reaction $H_2O_{(g)} \rightleftharpoons H_{2(g)} + \frac{1}{2}O_{2(g)}$ is endothermic $(\Delta H > 0)$.$4$. The reaction $4HCl_{(g)} + O_{2(g)} \rightleftharpoons 2H_2O_{(g)} + 2Cl_{2(g)}$ is exothermic.Therefore,increasing the temperature will shift the equilibrium in the forward direction for the endothermic reaction,which is option $C$.

If the temperature is increased,which of the following reactions will proceed in the forward direction?

Similar Questions

What is the effect of halving the pressure by doubling the volume on the following system at $500\,^{\circ}C$?
$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

Describe the effect of the following on the equilibrium of the reaction: $2H_{2(g)} + CO_{(g)} \rightleftharpoons CH_3OH_{(g)}$
$(a)$ Addition of $H_2$
$(b)$ Addition of $CH_3OH$
$(c)$ Removal of $CO$
$(d)$ Removal of $CH_3OH$

Select the correct statement from the following:

Two systems $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ and $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$ are in equilibrium simultaneously in a container of constant volume. If some $CO_{(g)}$ is added to the container at constant volume,then at the new equilibrium:

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