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# Calculate A) δG°And B) the Equilibrium Constant for the Formation of No2 from No and O2 at 298 K - CBSE (Science) Class 11 - Chemistry

ConceptLaw of Chemical Equilibrium and Equilibrium Constant

#### Question

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

NO(g) + 1/2 O_2 (g) "↔" NO_2(g)

where ΔfG° (NO2) = 52.0 kJ/mol

ΔfG° (NO) = 87.0 kJ/mol

ΔfG° (O2) = 0 kJ/mol

#### Solution

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

K_c = (-35.5xx10^(-3))/(-2.303xx8.314xx298)

= 6.134

:.. K_c = antilog (6.134)

= 1.36 xx  10^6

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

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#### APPEARS IN

Solution Calculate A) δG°And B) the Equilibrium Constant for the Formation of No2 from No and O2 at 298 K Concept: Law of Chemical Equilibrium and Equilibrium Constant.
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