The generic reaction 2 A B has the following rate laws where k_1 is the rate con

Question

The generic reaction 2 A B has the following rate laws where k_1 is the rate constant for the forward reaction and k_g is the rate constant for the reverse reaction. At equilibrium, the two rates are equal and so k[A]^2 = k[B] the equilibrium constant for a reaction is related by the law of mass action to the rate constants for forward and reverse reactions. Part A At a certain temperature the initial concentration of NO was 0.400 M and that of Br_2 was 0.245 M. At equilibrium the concentration of was found to be 0.250 M. What is the value of K_c at this temperature? Part B At this temperature the rate constant for the reverse reaction is 340. M^-1 s^-1. What is k_f for the reaction?

Explanation / Answer

Kc = 23.1

Kr = 340 M-1s-1

Kf = ?

Kc = Kf / Kr

23.1 = Kf / 340

Kf = 7854 M-1s-1

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