Determine the rate law and the value of k for the following reaction using the data provided.2 no(g) + o2(g) → 2 no2(g)[no]i (m)[o2]i (m)initial rate (m-2s-1)0.0300.00558.55 x 10-30.0300.01101.71 x 10-20.0600.00553.42 x 10-2

Rate law=

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 NO

y = order with respect to

n = x+y = Total order

a) From trial 1:    (1)

From trial 2:    (2)

Dividing 2 by 1 :

therefore y=1.

b) From trial 1 :   (3)

From trial 3: (4)

Dividing 4 by 3:

, x=2Thus rate law is

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

Rate law is

b) For calculating k:

Using trial 1:  

The value of rate constant is

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2