Hi guys, my question is:

Bromoethane is converted to methanol in an alkaline solution. This reaction is first order with respect to each reactant.

CH3Br (aq) + NaOH (aq) - -> CH3OH (aq) + NaBr (aq)

a) What is the rate law for this reaction?

b) Predict how the reaction rate will change when the concentration of NaOH is decreased by a factor of 5.

c) Predict the change in reaction rate when the concentrations of both reactant are doubled?

Question

Kamden Daniels

Chemistry

7 June, 06:19

Hi guys, my question is:

Bromoethane is converted to methanol in an alkaline solution. This reaction is first order with respect to each reactant.

CH3Br (aq) + NaOH (aq) - -> CH3OH (aq) + NaBr (aq)

a) What is the rate law for this reaction?

b) Predict how the reaction rate will change when the concentration of NaOH is decreased by a factor of 5.

c) Predict the change in reaction rate when the concentrations of both reactant are doubled?

+4

Answers (1)

Know the Answer?

Thomas Dunlap · Answer 1

See Explanation Below

Explanation:

A) The rate law can only be on the reactant side and you can only determine it after you get the net ionic equation because of spectators cancelling out. So in this case the rate law is k=[CH3Br]^1 [OH-]^1. The powers are there because the rxn is first order.

B) Since the rxn is first order anything you do to it will be the exact same "counter rxn" per say so since you are decreasing the OH - by 5 the rate will decease by 5

C) The rate will increase by 4 since you are doubling both you have to multiply them both.