## Chemistry 9th Edition

Rate = $k[C_4H_9Br]$ Overall balanced equation: $C_4H_9Br+2H_2O\rightarrow C_4H_9OH+Br^-+H_3O^+$ Intermediates: $C_4H_9^+$ and $C_4H_9OH_2^+$
The rate of the reaction is the rate of the slowest step, which is given in the problem. The overall balanced equation is found by adding the reactions of all 3 elementary steps given in the problem. The intermediates are the molecules produced and then consumed in the overall reaction. $C_4H_9^+$ is produced in the first elementary step and then consumed in the second while $C_4H_9OH_2^+$ is produced in the second elementary step and then consumed in the third.