Question

For the chemical reaction \(3 \mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons \mathrm{X}_{3} \mathrm{Y}(\mathrm{g})\) the amount of \(\mathrm{X}_{3} \mathrm{Y}\) at equilibrium is affected by (1) Tempcrature and pressure (2) Tempcrature only (3) Pressurc only (4) Temperature, pressure and catalyst

Short answer

The equilibrium amount of \(\mathrm{X}_3 \mathrm{Y}\) is affected by temperature and pressure, so the answer is (1).

Step-by-step solution

- Understand the Effect of Temperature

Determine how temperature affects the equilibrium of chemical reactions. According to Le Chatelier's Principle, if the reaction is exothermic (releases heat) or endothermic (absorbs heat), increasing or decreasing the temperature will shift the equilibrium position.

- Consider the Effect of Pressure

Evaluate how pressure changes impact the equilibrium. Le Chatelier's Principle states that an increase in pressure will shift the reaction towards the side with fewer gas molecules, and a decrease in pressure will shift it towards the side with more gas molecules.

- Think About the Role of a Catalyst

A catalyst speeds up the rate of reaction but does not affect the equilibrium position itself. However, it helps the system reach equilibrium faster.

- Analyze the Reaction Given

For the reaction \(3 \mathrm{X}(\mathrm{g})+\mathrm{Y}(\mathrm{g}) \rightleftharpoons \mathrm{X}_{3} \mathrm{Y}(\mathrm{g})\), there are 4 moles of gas on the reactant side and 1 mole of gas on the product side. Increasing pressure will shift the equilibrium to the right (towards fewer gas molecules). Temperature can also affect the equilibrium if the reaction is endothermic or exothermic.

- Conclusion

Based on the analysis, both temperature and pressure affect the equilibrium, and a catalyst speeds up the reaction but doesn't shift the equilibrium. Therefore, the correct choice must include temperature and pressure as factors.

Key concepts

Le Chatelier's Principle

Le Chatelier's Principle is a fundamental concept in chemical equilibrium. It states that if a system at equilibrium is disturbed by changing the conditions, the system will adjust itself to partially counteract that change and restore a new equilibrium. This principle helps predict how certain changes will affect the position of equilibrium in a chemical reaction.
For example:

• If the concentration of a reactant increases, the system will shift towards producing more products to reduce that concentration.
• If temperature is increased for an exothermic reaction, the system will shift towards the reactants to absorb the added heat.

This principle is very useful in understanding and predicting the behavior of reactions involving gases.

Effect of Temperature on Equilibrium

Temperature changes can significantly impact the position of equilibrium in a chemical reaction. According to Le Chatelier's Principle, the system will adjust to minimize the effect of the temperature change. If a reaction is exothermic (releases heat), increasing the temperature will drive the equilibrium towards the reactants. Conversely, if the reaction is endothermic (absorbs heat), increasing the temperature will favor the formation of products.
Consider the example reaction: