Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimental data provided. (4 points) a + b yieldsproducts trial [a] [b] rate 1 0.10 m 0.20 m 1.2 × 10-2 m/min 2 0.10 m 0.40 m 4.8 × 10-2 m/min 3 0.20 m 0.40 m 9.6 × 10-2 m/min

Rate law=, order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

k= rate constant

x = order with respect to A

y = order with respect to A

n = x+y = Total order

a) From trial 1:    (1)

From trial 2:    (2)

Dividing 2 by 1 :

therefore y=2.

b) From trial 2:    (3)

From trial 3:   (4)

Dividing 4 by 3:

, x=1

Thus rate law is

Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.

c) For calculating k:

Using trial 1:  

.

false

because it does not have the potential to be entirely used up