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Question

Calculate

Δ G0

the equilibrium constant for the formation of NO2 from NO and O2 at 298 K
NO(g)+12O2(g)NO2(g)

Where:
ΔfG (NO2)=52.0kJ/molΔfG (NO)=87.0kJ/molΔfG (O2)=0kJ/mol

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Solution

Fort the given reaction,
ΔG=ΔG (Products ) - ΔG (Reactants)
ΔG=52.0{87.0+0}=35.0 kJ mol1(or)35×103 J mol1

We know that,
ΔG=RT log Kc
ΔG=2.303RT log Kc
Kc=35.0×1032.303×8.314×298=6.134 Kc=antilog(6.134)=1.36×106
Hence, the equilibrium constant for the given reaction Kc is 1.36×106


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