Consider the following reversible first order reaction of X at an initial concentration X 0 . The values of the rate constants are K f = 2   s - 1 and K b = 1   s - 1 X ⇌ K b K f Y A plot of concentration of X and Y as function of time is

Step-by-step solution

For first order reaction, X ⇌ Y Given, K f = 2   s - 1 K b = 1   s - 1 ∴ K eq = K f K b = Y X K eq = 2 1 = Y X ⇒ 2 X = Y or 2 X eq = Y eq ∴ Y > X Thus, as the rate of reaction increases, there will be increased in the concentration Y eq , but it will be less than initial concentration of X X 0 , whereas the concentration of X eq decreases.