For the equilibrium C_{(diamond)} rightleftha | vedclass

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(A) According to Le Chatelier's principle,increasing the pressure favors the direction in which the volume decreases (or density increases). Density i

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The backward reaction is favored.

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(A) According to Le Chatelier's principle,increasing the pressure favors the direction in which the volume decreases (or density increases). Density is defined as $	ext{Density} = \frac{	ext{Mass}}{	ext{Volume}}$,which implies $	ext{Volume} = \frac{	ext{Mass}}{	ext{Density}}$. Since the density of diamond $(3.5 \ g/mL)$ is greater than that of graphite $(2.3 \ g/mL)$,the volume of $1 \ g$ of diamond is less than the volume of $1 \ g$ of graphite. Therefore,increasing the pressure shifts the equilibrium towards the side with the smaller volume,which is the diamond side. Thus,the backward reaction is favored.

For the equilibrium $C_{(diamond)} \rightleftharpoons C_{(graphite)}$,the densities of diamond and graphite are $3.5 \ g/mL$ and $2.3 \ g/mL$ respectively. What happens to the equilibrium upon increasing the pressure?

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