Question
The unit of rate constant for the reaction, $$2{H_2} + 2NO \to 2{H_2}O + {N_2}$$
which has rate $$ = k\left[ {{H_2}} \right]{\left[ {NO} \right]^2},$$ is
A.
$$mol\,{L^{ - 1}}\,{s^{ - 1}}$$
B.
$${s^{ - 1}}$$
C.
$$mo{l^{ - 2}}\,{L^2}\,{s^{ - 1}}$$
D.
$$mol\,{L^{ - 1}}$$
Answer :
$$mo{l^{ - 2}}\,{L^2}\,{s^{ - 1}}$$
Solution :
Unit of rate constant for the reaction is
$$\eqalign{
& k = \frac{{{\text{rate}}}}{{\left[ {{H_2}} \right]{{\left[ {NO} \right]}^2}}} \cr
& \,\,\,\, = \frac{{mol\,{L^{ - 1}}\,{s^{ - 1}}}}{{\left( {mol\,{L^{ - 1}}} \right){{\left( {mol\,{L^{ - 1}}} \right)}^2}}} \cr
& \,\,\,\, = mo{l^{ - 2}}\,{L^2}\,{s^{ - 1}} \cr} $$