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Question
Find out the value of the equilibrium constant for the following reaction at 298 K, \[\ce{2NH3_{(g)} + CO2_{(g)} ⇌ NH2CONH2_{(aq)} + H2O_{(l)}}\] Standard Gibbs energy change, `∆"G"_"r"^0` at the given temperature is –13.6 kJ mol−1.
Solution
Given, T = 298 K
`∆"G"_"r"^0` = –13.6 kJ mol−1
= −13600 J mol−1
ΔG0 = − 2.303 RT log Keq
log Keq = `(-Δ"G"^0)/(2.303 "RT")`
log Keq = `(13.6 "kJ mol"^-1)/(2.303 xx 8.314 xx 10^-3 "JK"^-1 "mol"^-1 xx 298 "K")`
log Keq = 2.38
Keq = antilog (2.38)
Keq = 239.88
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