Question

The activation energy for forward and backward reactions are $50kJ/mol$ and $40kJ/mol$ respectively. If ${K_1}$ ​ and ${K_2}$ ​ are the equilibrium constants of reaction at temperature ${T_1}$ ​ and ${T_2}$ ​ respectively and ${T_2} > {T_1}$ then:
(A) ${K_1} < {K_2}$
(B) ${K_1} = {K_2}$
(C) ${K_1} > {K_2}$
(D) ${K_2} = {K_1}^2$

Answer 1

To solve this question, we must first understand the basic concepts about Chemical Equilibrium and Activation Energy. Then we need to assess the compounds that are used in the formation of wine and then only we can conclude the correct answer.

Complete step-by-step solution: Before we move forward with the solution of this given question, let us first understand some basic concepts:
Chemical equilibrium: It refers to the state of a system in which the concentration of the reactant and the concentration of the products do not change with time and the system does not display any further change in properties.
Activation energy is defined as the minimum amount of extra energy required by a reacting molecule to get converted into a product. It can also be described as the minimum amount of energy needed to activate or energize molecules or atoms so that they can undergo a chemical reaction or transformation.
The activation energy for forward and backward reactions are $50kJ/mol$ and $40kJ/mol$ respectively. If ${K_1}$ ​ and ${K_2}$ ​ are the equilibrium constants of reaction at temperature ${T_1}$ ​ and ${T_2}$ ​ respectively and ${T_2} > {T_1}$ then ${K_1} < {K_2}$
The equilibrium constant at higher temperatures is higher than the equilibrium constant at lower temperatures.
$\Delta H = {E_f} - {E_b} = 50 - 40 = 10{\text{ }}kJ/mol$
Since, the value of Enthalpy change is positive therefore it reflects the endothermic nature. And in endothermic reactions, equilibrium constant increases with an increase in temperature.

So, clearly we can conclude that the correct answer is Option (A).

Note: Endothermic reactions are chemical reactions in which the reactants absorb heat energy from the surroundings to form products. These reactions lower the temperature of their surrounding area, thereby creating a cooling effect.