Question

For a chemical reaction $3\left(g\right)+Y\left(g\right)\leftrightharpoons X_3{Y}_{\left(g\right)}$, the amount of $X_{3}Y$, at equilibrium is affected by:

• A. temperature and pressure
• B. temperature only
• C. pressure only
• D. temperature, pressure and catalyst

Answer 1

The correct option is A temperature and pressure

Given reaction-

$3\times \left(g\right)+Y\left(g\right)\rightleftharpoons X_{3}Y\left(g\right)$ is a synthesis reaction.

no. moles reactant $=(3+1)=4$

no. moles product $=1$

According to Lechatelier's Principle-

$Pressure$: Increasing pressure shifts equilibrium to the side of reaction with fever moles of gaseous molecules. In this case, increasing pressure will shift the equilibrium to right.

$Temperature$: The given reaction is a synthesis reaction. Synthesis reactions release energy, so they are exothermic.

Increasing the temperature will cause the equilibrium to shift towards the product side.

$Catalyst$: catalysts speed up the reactions, but have no effect on the equilibrium.

Hence, the correct option is A