Courses
Courses for Kids
Free study material
Offline Centres
More
Store Icon
Store
seo-qna
SearchIcon
banner

For endothermic reaction when a change in entropy is negative, then the reaction is:
A.Not possible at any temperature
B.Possible at low temperature
C.Possible at all temperature
D.Possible at high temperature

Answer
VerifiedVerified
488.1k+ views
1 likes
like imagedislike image
Hint: Those chemical reactions in which there is absorption of heat energy by the reactants from the surroundings to form products are called endothermic reactions. In case of endothermic reactions, the enthalpy change is positive. From the enthalpy change and the entropy change, the change in free energy which decides the spontaneity of the chemical reaction can be determined.

Complete step by step answer:
The enthalpy change of an endothermic reaction is positive because the enthalpy of the products is greater than that of the reactants as there is absorption of heat. In other words, ΔH = + ve.
Entropy is the property of a system which measures the randomness or the amount of disorder of a system quantitatively. Greater the randomness of the system, greater is the entropy. It is a state function just like internal energy and enthalpy because the magnitude of its change also depends on the entropies of the system in the initial and final states. Now, according to the given question, change in entropy is negative. In other words, ΔS = - ve.
According to the Gibbs Helmholtz equation, the change in the free energy of a system is related to the change in enthalpy as well as the change in entropy by the relation:
ΔG=ΔH - TΔS
Here, T is the temperature of the system.
The Gibbs free energy concept is useful in determining the spontaneity or the feasibility of a process. The process will be spontaneous if ΔG is negative and non-spontaneous when ΔG is positive.
Now, for the given endothermic reaction, ΔH = + ve and ΔS = - ve. From the Gibbs Helmholtz equation, we see that if ΔS = - ve, then the term TΔS is also negative.
Thus, we will have:
ΔG = ( + ve) - ( - ve)ΔG = + ve
Hence, free energy change is positive. Thus, the process is not spontaneous and is not possible at any temperature.

So, the correct option is A.

Note:
If both ΔH = + ve and ΔS = + ve, then free energy change is positive when ΔH is greater than TΔS and the reaction will be non-spontaneous. The free energy change is negative when ΔH is less than TΔS and the reaction will be spontaneous.
If ΔH = - ve and ΔS = - ve, then free energy change is negative when ΔH is greater than TΔS and the reaction will be and the reaction will be spontaneous. The free energy change is positive when ΔH is less than TΔS and the reaction will be non-spontaneous.