Question

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO2 for this period is __________.

Answer 1

`rate=-1.75x10^(-5)(M)/(s)`

Step-by-step explanation:

Hello,

In this case, for the given information, we can compute the rate of disappearance of NO₂ by using the following rate relationship:

`rate=(1)/(2)*(C_f-C_0)/(t_f-t_0)`

Whereas it is multiplied by the the inverse of the stoichiometric coefficient of NO₂ in the reaction that is 2. Moreover, the subscript f is referred to the final condition and the subscript 0 to the initial condition, thus, we obtain:

`rate=(1)/(2)*(0.00650M-0.0100M)/(100s-0s)\\\\rate=-1.75x10^(-5)(M)/(s)`

Clearly, it turns out negative since the concentration is diminishing due to its consumption.

Regards.