Question

use this information to write a rate law for this reaction and calculate the value of the rate constant k

= Knowledge Check Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H.] initial rate of reaction 0.938 M 1.30 M 0.822 M/S 0.938 M 5.72 M 15.9 M/S 0.138 M 1.30 M 0.0178 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate - 1 XI ?

Answer 1

1)

see experiment 3 and 1:

[N2] becomes 6.8 times

[H2] is constant

rate becomes 46.2 times

Since 6.8^2 = 46.2, order of N2 is 2

see experiment 1 and 2:

[N2] is constant

[H2] becomes 4.4 times

rate becomes 19.4 times

Since 4.4^2 = 19.4, order of H2 is 2

Rate law is:

rate = k*[N2]^2*[H2]^2

Answer:

rate = k [N2]^2 [H2]^2

2)

Put values from 1st row of table in rate law

rate = k*[N2]^2*[H2]^2

0.822 = k*0.938^2*1.3^2

k = 0.553 M-3.s-1

Answer: 0.553 M-3.s-1