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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

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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

  Is there an error in this question or solution?

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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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