Question

For the given reaction at equilibrium $ 2S{O_2}\,(g)\, + \,{O_2}\,(g)\, \rightleftharpoons \,2S{O_3}\, + \,189.4\,KJ $ what would be the effect on equilibrium if
(A) Pressure is increased
(B) Temperature is increased

Answer 1

Hint: Let us first get some idea about the Le chatelier’s principle. When a system encounters a disruption (such as concentration, temperature, or pressure changes), Le Chatelier's principle (also known as "Chatelier's principle" or "The Equilibrium Law") states that it will act to restore a new equilibrium state.

Complete answer:
Effect of pressure:
 $ 2S{O_2}\,(g)\, + \,{O_2}\,(g)\, \rightleftharpoons \,2S{O_3}\, + \,189.4\,KJ $
As pressure is raised, the equilibrium moves to the side with the fewer moles of gas, according to Le Chatelier's principle. This particular reaction shows a total of $ 3\,mol $ of gas as reactants and $ 2\,mol $ of gas as products, so the reaction shifts towards the product side.
Effect of temperature:
The heat of reaction is what determines how temperature affects equilibrium. Remember that in an endothermic reaction, heat is consumed, and $ \vartriangle H $ is positive. As a result, we can think of heat as a reactant in an endothermic reaction:
 $ heat\, + \,A\, \rightleftharpoons B\,\,\vartriangle H = + $
The condition is the polar opposite with an exothermic reaction. Since heat is emitted during the reaction, it is a gas, and the value of $ \vartriangle H $ is negative:
 $ A\, \rightleftharpoons \,B\, + \,heat\,\,\vartriangle H = \, - $
If we think of heat as a reactant or a substance, we can use Le Chatelier's theory to raise or lower concentrations, just as we did in our previous discussion. For example, increasing the temperature of an endothermic reaction is basically the same as introducing more reactant to the system, so the equilibrium would change to the right according to Le Chatelier's theory. Lowering the temperature in an endothermic reaction, on the other hand, would change the equilibrium to the left, so lowering the temperature is equal to removing a reactant in this situation.
Heat is a result of an exothermic reaction. As a result, increasing the temperature causes the equilibrium to shift to the left, thus lowering the temperature causes the equilibrium to shift to the right.

Note:
Let’s see a little more about equilibrium. Equilibrium is a crucial principle since it ensures consistency. When a chemical reaction enters equilibrium, for example, the chemicals become stable, allowing us to predict and depend on the products' reactions.