Question

Assertion: For an exothermic reaction, the extent of reaction increases with increase in temperature.
Reason: With increase in temperature, the rate of forward reaction increases more.
A.Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
B.Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion.
C.Assertion is correct but Reason is incorrect
D.Both Assertion and Reason are incorrect

Answer 1

Hint: Exothermic reactions are those reactions which evolve heat as the reaction proceeds, that is heat is one of the products of these reactions. When the amount of reactant is increased in a reaction, the reaction tries to move towards equilibrium position thereby increasing the amount of product.

Complete step by step answer:
As said earlier exothermic reactions are the reactions in which evolution of heat takes place as the reaction proceeds. So, for the reaction to move forward the amount of reactant can be increased as the reaction will try to attain equilibrium and the formation of product will be favoured.
For exothermic reactions, increasing the temperature means increasing the amount of product, so the reaction will try to attain equilibrium, thereby increasing the amount of reactant. Hence, favouring backward reaction.
Increasing the temperature of a reaction cannot itself determine if the rate of forward reaction increases or backward without knowing whether the reaction is endothermic or exothermic.
Therefore, both assertion and reason are incorrect.

So, the correct answer is option D.

Note:
We can deduce from the above explanation that for an exothermic reaction, if we want to increase the rate of forward reaction then the temperature of the reaction should be decreased. So that to compensate the decrease in temperature formation of products is favoured as a result of which heat will be liberated.