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(A) According to Le Chatelier's principle,for a gaseous reaction,an increase in the volume of the container shifts the equilibrium towards the side wi

Vedclass · Accepted Answer

$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

Vedclass · Answer

(A) According to Le Chatelier's principle,for a gaseous reaction,an increase in the volume of the container shifts the equilibrium towards the side with a greater number of moles of gaseous species.Mathematically,the yield of products $(x)$ is proportional to $V^{\Delta n_g}$,where $\Delta n_g = (	ext{moles of gaseous products}) - (	ext{moles of gaseous reactants})$.If $\Delta n_g > 0$,an increase in volume $(V)$ increases the formation of products.						Reaction			$\Delta n_g$							$A$. $C_{(s)} + H_2O_{(g)} ightleftharpoons CO_{(g)} + H_{2(g)}$			$\Delta n_g = (1+1) - 1 = 1$							$B$. $H_{2(g)} + I_{2(g)} ightleftharpoons 2HI_{(g)}$			$\Delta n_g = 2 - (1+1) = 0$							$C$. $4NH_{3(g)} + 5O_{2(g)} ightleftharpoons 4NO_{(g)} + 6H_2O_{(l)}$			$\Delta n_g = 4 - (4+5) = -5$							$D$. $3O_{2(g)} ightleftharpoons 2O_{3(g)}$			$\Delta n_g = 2 - 3 = -1$			Since $\Delta n_g > 0$ only for reaction $A$,an increase in volume will favour the formation of products in reaction $A$.

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

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