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 0.477 M, the concentration of NO2 will be
M after 12.4 seconds have passed.

Answer 1

`[NO_2]=0.112M`

Step-by-step explanation:

Hello there!

In this case, since the second-order integrated law is given by the following equation:

`(1)/([NO_2]) =(1)/([NO_2]_0)+kt`

Thus, given the initial concentration of the nitrogen dioxide gas, the rate constant and the elapsed time, we obtain:

`(1)/([NO_2])= (1)/(0.477M) +0.54M^(-1)s^(-1)\\\\(1)/([NO_2])=8.933M^(-1)`

`[NO_2]=(1)/(8.933M^(-1)) =0.112M`

Best regards!