For the reaction 3X_{(g)} + Y_{(g)} rightleft | vedclass

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(A) According to Le Chatelier's principle,the equilibrium position of a reaction is affected by changes in temperature and pressure if there is a

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Temperature and pressure

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(A) According to Le Chatelier's principle,the equilibrium position of a reaction is affected by changes in temperature and pressure if there is a change in the number of moles of gaseous species.
In the given reaction: $3X_{(g)} + Y_{(g)} \rightleftharpoons X_3Y_{(g)}$,the number of moles of gaseous reactants is $4$ $(3+1)$ and the number of moles of gaseous products is $1$.
Since there is a change in the number of moles $(\Delta n_g = 1 - 4 = -3)$,the equilibrium will be affected by pressure.
Additionally,the equilibrium constant $K_c$ is temperature-dependent,so temperature changes will shift the equilibrium position.
$A$ catalyst only increases the rate of both forward and backward reactions equally and does not affect the equilibrium position or the amount of products at equilibrium.
Therefore,the amount of $X_3Y$ is affected by temperature and pressure.

For the reaction $3X_{(g)} + Y_{(g)} \rightleftharpoons X_3Y_{(g)}$,the amount of $X_3Y$ at equilibrium is affected by ...........

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