Chemistry, asked by vidhyasree35, 11 months ago

a). For the reaction
2A (8) + B (E) – 2D
AU' = - 10.5 KJ and AS* = -44.10 JK
Calculate AG for the reaction and predict, whether the reaction may
occur spontaneous

Answers

Answered by abinayaasrisureshlv
0

Answer:

For the given reaction

2A

(g)

+B

(g)

⟶2D

(g)

Δn

g

=2−3=−1mole

Substituting the value of ΔU

θ

in the expansion of ΔH :

ΔH

θ

=ΔU

θ

+Δn

g

RT

=(−10.5kJ)+(+1)(8.314×10

−3

kJK

−1

)(298K)

=−10.5kJ−2.48kJ

=−12.98kJ

When we substitute the values of ΔH

θ

and ΔS

θ

in the expression of ∣deltaG

θ

then according to Gibbs' Helmholtz equation

ΔG

θ

=ΔH

θ

−TΔS

θ

=−12.98kJ−(298K)(−44.1JK

−1

)

=−12.98kJ−(13.14kJ)

ΔG

θ

=0.16kJ

Since ΔG

θ

for the reaction is positive , the reaction will not occur spontaneously .

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