an explanation along with the related answer/work would help and be appreciated.

Question

an explanation along with the related answer/work would help and be appreciated. . we have to explain our answers on our exams. (he loves detail related laws, rules. etc)

13.62 The following data were collected for the reaction:

H2(g) + NO(g) ? N2O(g) + H2O(g)

experiment initial [H2]0 initial [NO]0 initial rate (M/s)

1 0.35 0.30 2.835x 10-3

2 0.35 0.60 1.134 x 10 -2

3 0.70 0.60 2.268 x 10 -2

Determine the rate law and the rate constant for the reaction at the temperature for which the data were collected.

Explanation / Answer

see experiment 2 and 3:

[H2] doubles

[NO] is constant

rate doubles

so, order of H2 is 1

see experiment 1 and 2:

[H2] is constant

[NO] doubles

rate becomes 4 times

so, order of NO is 2

overall order = 1 + 2 = 3

Rate law is:

rate = k*[H2]*[NO]^2

Put values from 1st row of table in rate law

rate = k*[H2]*[NO]^2

2.835*10^-3 = k*0.35*0.3^2

k = 0.0900 M-2.s-1

Answer:

rate = k*[H2]*[NO]^2

K = 0.0900 M-2.s-1

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