SELECT * FROM question_mgmt as q WHERE id=3048 AND status=1 SELECT id,question_no,question,chapter FROM question_mgmt as q WHERE courseId=2 AND subId=9 AND chapterId=48 and ex_no='1' AND status=1 ORDER BY CAST(question_no AS UNSIGNED) CBSE Free NCERT Solution of 11th chemistry Equilibrium calculate a delta g0 and b the equilibrium cons

Question:

Calculate a) ΔG0 and b) the equilibrium constant for the formation of NO2 from NO and O2 at 298K

NO (g) + ½ O2 (g) ↔ NO2 (g)

where ΔfG0 (NO2) = 52.0 kJ/mol

ΔfG0 (NO) = 87.0 kJ/mol

ΔfG0 (O2) = 0 kJ/mol

Answer:

(a) For the given reaction,

ΔG° = ΔG°( Products) - ΔG°( Reactants)

ΔG° = 52.0 -{87.0 + 0} = -35.0 kJ mol-1

(b) We know that,

ΔG° = RT log Kc

ΔG° = 2.303 RT log Kc

Hence, the equilibrium constant for the given reaction Kc is 1.36 × 106


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