SELECT * FROM question_mgmt as q WHERE id=2807 AND status=1 SELECT id,question_no,question,chapter FROM question_mgmt as q WHERE courseId=2 AND subId=9 AND chapterId=47 and ex_no='1' AND status=1 ORDER BY CAST(question_no AS UNSIGNED)

Question:

For the reaction

2 A(g) + B(g) → 2D(g)

ΔU0 = –10.5 kJ and ΔS0 = –44.1 JK–1.

Calculate ΔG0 for the reaction, and predict whether the reaction may occur spontaneously.

Answer:

For the given reaction,

2 A(g) + B(g) → 2D(g)

Δng = 2 - (3) = -1 mole

Substituting the value of ΔU0¸ in the expression of ΔH:

ΔHº  = ΔUº + ΔngRT

= (-10.5 kJ) - (-1) (8.314 x 10-3 kJ K-1 mol-1) (298 K)

= -10.5 kJ - 2.48 kJ

ΔHº  =  -8.02 kJ

Substituting the values of ΔHº and ΔSº¸ in the expression of ΔH:

ΔGº  =  ΔHº  - TΔSº

= -8.-02 kJ - (298 K) (-44.1 J K-1)

= -8.02 kJ + 13.14 kJ

ΔGº = + 5.12 kJ

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


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