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Question

For a general reaction aA(g) + bB(g) cC(g)+ dD(g), what is the relationship between the equilibrium constants Kc and Kp? [assume Δn = μ = (c + d) - (a+b)


A

Kp = Kc (RT)Δn

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B

Kc = Kp (RT)Δn

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C

KpKc = 1

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D

Kp = Kc

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Solution

The correct option is B

Kc = Kp (RT)Δn


For the reactionaA(g) + bB(g) cC(g) + dD(g)

Kp = (Pc)c(Pd)d(Pa)a(Pb)b
From Dalton's law of partial pressure,
PA = [A]RT; PB = [B]RT; PC = [C]RT; PD = [D]RT
Substituting the above in the expression for Kp, we get
Kp = Kc (RT)Δn or Kc = Kp (RT)Δn
where Δn = sum of coefficients of gaseous products - sum of coefficients of gaseous reactants = (c + d) - (a+b)
Hence options a and b


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