For the reversible, one-step reaction A + B ARROW C + D, the forward rate constant is 35.9 1/(M·h) and the rate constant for the reverse reaction is 25.4 1/(M·h). The activation energy was found to be 33.0 kJ/mol for the forward reaction and 45.6 kJ/mol for the reverse reaction.

What is the equilibrium constant for the reaction?

To determine the equilibrium constant for the reaction, we can use the relationship between the rate constants and the equilibrium constant.

The equilibrium constant (K) for the reaction can be expressed as the ratio of the rate constant for the forward reaction (k forward) to the rate constant for the reverse reaction (k reverse). Mathematically, it can be written as:

K = (k forward) / (k reverse)

In this case, the forward rate constant (k forward) is given as 35.9 1/(M·h), and the reverse rate constant (k reverse) is given as 25.4 1/(M·h).

Substituting these values into the equation, we have:

K = 35.9 / 25.4

Calculating this value, we find:

K ≈ 1.41

Therefore, the equilibrium constant for the reaction is approximately 1.41.