Question

For the reaction at 25oC,X2O4(l)⟶2XO2(g) ΔH=2.1kcal and ΔS=20calK−1. The reaction would be: A spontaneous B non-spontaneous C at equilibrium D unpredictable

Answer 1

Answer:

Hello mate ✌️

Explanation:

The change in Gibbs Free energy is given by

ΔH=ΔU+Δn

g

RT

where

ΔH is the enthalpy of the reaction

ΔS is the entropy of the reaction

and ΔU is the change in internal energy

Δn

g

is the (number of gaseous moles in product) - (number of gaseous moles in reactant)=2-0=2

R is the gas constant =2 cal

But,

ΔH=(2.1×10

3

)+(2×2×300)=3300cal

Hence,

ΔG=ΔH=TΔS

ΔG=3300−(300×20)

ΔG=−2700cal=−2.7cal

hope it will be helpful to you ✌️

itz Essar 03 ❤️

Answer 2

as change in entropy is +ve ...so given rxn ( which is not clear ) must be spontaneous