How can you determine the rate law of the following reactions?
`2NO(g) + O_(2)(g) to 2NO_(2)(g)`

Explanation

The rate law can be determined by 'initial rate method' (page `4//31`, 32). Keeping the concentration of one of the reactants constant and changing the concentration of the other, the effect on the rate of reaction is determined. For example, for the given reaction,
(i) Keeping `[O_(2)]` constant, if `[NO]` is doubled, rate is found to become four times. This shows that
Rate `prop[NO]^(2)`.
(ii) Keeping [NO] constant, if `[O_(2)]` is doubled, rate is also found to become double. This shows that
Rate `prop[O_(2)].`
Hence, overall rate law will be : Rate `=k[NO]^(2)[O_(2)]`.