The table below contains concentration and rate data for a reaction involving three reactants. Use these data to determine the overall order of the reaction and the order with respect to M, N, and P.

The order of reaction with respect to M, N, and P are 1, 0, and 3, respectively.

The overall order of reaction is 4.

Explanation:

We are given a table containing the concentrations of M, N, P, and the rate of the reaction, and we want to determine the overall order of the reaction and the order with respect to each reactant.

To do so, we can select two experiments from the list where two of the reactant concentrations are held constant and only one changes.

From trials 1 and 2, we can see that holding [N] and [P] constant while doubling [M] doubles the rate.

Therefore, because the rate is directly proportional to M, the reaction is first order with respect to M.

From trials 2 and 3, we can see that holding [M] and [P] constant while doubling [N] does not affect the rate.

Therefore, the reaction is zero order with respect to N.

From trials 1 and 4, we can see that holding [M] and [N] constant and doubling [P] leads to a eight-fold increase (2.6/0.32 ≈ 8).

Therefore, the reaction is third order with respect to P (2³ = 8).

Hence, our rate law is:

Where the order of reaction with respect to M, N, and P are 1, 0, and 3, respectively.

And the overall order is the sum of each individual reaction orders, or 4.

c. 4.54 x 10–12 j happens to be correct