Question

The value of the rate constant for the gas phase reaction, $2N{O}_2+F_2\to 2N{O}_{2}F$ is $38d{m}^{3}mo{l}^{-1}{s}^{-1}$ at 300K. The order of the reaction is:

• A. 0
• B. 1
• C. 2
• D. 3

Answer 1

The correct option is C

2

The reaction is not first order for sure, that would have a unit of $s^{-1}$.
For all other orders, unit of rate constant: $[conc.{]}^{1-n}{s}^{-1}$

If $n=2$

It will be $(mold{m}^{-3}{)}^{1-2}{s}^{-1}$

$\Rightarrow mo{l}^{-1}d{m}^{+3}{s}^{-1}$