Question

The gas phase decomposition of nitrogen dioxide at 383 °C NO2(g) --> NO(g) + ½ O2(g) is second order in NO2 with a rate constant of 0.540 M-1 s-1. If the initial concentration of NO2 is 0.355 M, the concentration of NO2 will be ______ M after 15.9 seconds have passed.

Answer 1

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Step-by-step explanation:

Integrated rate law for second order kinetics is:

`(1)/([A_t]) = (1)/([A]_0)+kt`

Where,
`[A_t]` is the final initial concentration

`[A_0]` is the initial concentration = 0.355 M

k is the rate constant = 0.540 (Ms)⁻¹

t is the time = 15.9 seconds

Applying the values in the above expression as:-

`(1)/([A_t]) = (1)/(0.355)+0.540* 15.9\ M=11.4\ M`

11.4 M of
`NO_2` will be left after 15.9 seconds have passed.