Chemistry, asked by ImRitz6981, 11 months ago

A particular reaction is spontaneous upto 475k and becomes non-spontaneous at temperatures above 475k. (i) is this reaction exothermic or endothermic?

Answers

Answered by BarrettArcher
18

Answer : This reaction is exothermic reaction.

Explanation :

According to Gibbs's equation:

\Delta G=\Delta H-T\Delta S

\Delta G = Gibbs free energy  

\Delta H = enthalpy change

\Delta S = entropy change  

T = temperature in Kelvin

When \Delta G is positive then the reaction is non spontaneous.

When \Delta G is negative then the reaction is spontaneous.

When \Delta G is equal to 0 then the reaction is in equilibrium.

As per question,

At low temperature (upto 475 K) and at high temperature (above 475 K), the reaction is spontaneous and non-spontaneous respectively, that means the value of \Delta H = -ve and the value of \Delta S = -ve.

When the value of \Delta H = -ve and the value of \Delta S = -ve then the reaction will be exothermic.

Hence, the reaction is exothermic reaction.

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