Question

The initial rate data for the reaction 2N₂O_5(g) → 4NO_2(g) + O_2(g) is shown in the following table.

            Experiment    [N₂O₅](M)        Rate (M/s)

                1         1.28 × 10²         22.5

                2         2.56 x 10²         45.0

a. Determine the order of reaction of the given reactant.

b. Determine the value of the rate constant for this reaction.

Answer 1

(a) rate law expression can be given as follows

$rate=k[N_2O_5]^a ......................(i)$

$22.5=k[1.28\times 10^2]^a ......................(i)$

$45=k[2.56\times 10^2]^a ......................(ii)$

dividing (ii) by (i)

$2=[2]^a$

On compairing both

value of a is 1

order of reaction

for finding rate constant use equation 1

(b)

$45=k[2.56\times 10^2]^1$

$k= 17.578 \times 10^{-2} s^{-1}$

$k= 1.76 \times 10^{-1} s^{-1}$