For the equilibrium process H_2O_{(l)} rightl | vedclass

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(B) According to $Le \ Chatelier's \ principle$,if the pressure is increased on a system at equilibrium,the system will shift in the direction that re

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The equilibrium shifts in the backward direction.

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(B) According to $Le \ Chatelier's \ principle$,if the pressure is increased on a system at equilibrium,the system will shift in the direction that reduces the number of moles of gas.In the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$,the product side has $1 \ mole$ of gas,while the reactant side has $0 \ moles$ of gas.Increasing the pressure favors the formation of the liquid phase (the side with fewer moles of gas).Therefore,the equilibrium shifts in the backward direction.

For the equilibrium process $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$,what happens if the pressure is increased?

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