Consider the reaction of chloromethane with OH- in aque- ous solu...

Question

Consider the reaction of chloromethane with OH- in aque- ous solution: 
CH Cl1aq2 + OH-1aq2 ∆kf CH OH1aq2 + Cl-1aq2 
At 25 °C, the rate constant for the forward reaction is 6 * 10-6 M-1 s-1, and the equilibrium constant Kc is 1 * 1016. Calculate the rate constant for the reverse reac- tion at 25 °C.

Accepted Answer

Hello. In this problem we are told that 27°C acquis reaction between methanol and hydrodynamic acid is as follows. We asked what is the rate constant for the reverse reaction? You have to break constant for the forward reaction And the equilibrium constant at 27° are 1.67 times 10 -4 per concentration per second, And 1.20 times 10-2. Respectfully. So recall we can write our equilibrium constant as K forward over K reverse. So we then can isolate reverse. We multiply both sides by reverse, cancels on the right hand side and then we divide both sides by our equilibrium constant. So our reaction rate constant for the forward reaction we were told was 1.67 times 10 to the -4 per concentration per second And our equilibrium constant is equal to 1.20 times 10 to the two. This gives us the reaction rate constant for the reverse reaction Being 1.39 Times 10 to the -6 per concentration per second. So making use of the fact that the equilibrium constant is equal to K forward over K reverse. You can rewrite the equation to solve for K. Reverse turns out that the reaction rate constant for the reverse reaction is equal to 1.39 times 10 to minus six per concentration per second. Thanks for watching. Hoping to help

Watch next