Suppose that the gas-phase reaction A B and B A are both elementary processes wi

Question

Suppose that the gas-phase reaction A B and B A are both elementary processes with rate constants of 4.91e-04 s-1 and 5.32e-03 s-1, respectively. Figure out the value of the equilibrium constant, KP, for the equilibrium A(g) B(g), and figure out which of the two substances, A or B develops higher partial pressure at equilibrium. Use this information to pick the choice from below which is correct. a) KP = 1.08e+01, and A(g) develops higher partial presssure. b) KP = 4.83e-03, and A(g) develops higher partial presssure. c) KP = 9.23e-02, and A(g) develops higher partial presssure. d) KP = 4.83e-03, and B(g) develops higher partial presssure. e) KP = 1.08e+01, and B(g) develops higher partial presssure.

Explanation / Answer

The answer is: a) KP = 1.24e-01, and A(g) develops higher partial presssure.

A(g) <=> B(g)

Rate constant of forward reaction = k1 = 5.40 x 103 s-1

Rate constant of reverse reaction = k-1 = 4.35 x 104 s-1

At equilibrium, forward rate = reverse rate

k1 x P(A) = k-1 x P(B)

Equilibrium constant Kp = P(B)/P(A)

= k1/k-1

= 5.40 x 103/4.35 x 104

= 1.24 x 10-1 = 1.24e-01

P(B) = 1.24 x 10-1 x P(A)

Thus P(B) < P(A) and A(g) develops higher partial presssure

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