Question

enthalpy and entropy changes of a reaction are 40.63 KJ mol -1 and 108.8JK-1 MOL -1 respectively .predict the feasibility of the reaction at 27degree cel.

Answer 1

Answer: Non spontaneous

Explanation:

Using Gibbs Helmholtz equation:

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

Given: T= Temperature = $27^0C=27+273=300 K$

$\Delta H$= enthalpy change = 40.63 kJ/mol  = 40630 J/mol

$\Delta S$= entropy change=  108.8 J/Kmol

Putting the values  the equation:

$\Delta G=40630-300(108.8)$

$\Delta G=7990Joules$

when $\DeltaG$= +ve, reaction is non spontaneous

$\DeltaG$= -ve, reaction is spontaneous

$\DeltaG$= 0, reaction is in equilibrium

As the value of $\Delta G$ comes out to be positive, the reaction is non spontaneous at $27^0C$.

Answer 2

Answer:

ans is 7990...

Explanation:

hope help you.....