For the reaction

$2H_2 + 2NO \to N_2 + 2H_2O$

the following mechanism has been proposed

$(i)$  $2NO \rightleftharpoons N_2O_2\,$   (fast)

$(ii)$ $N_2O_2 + H_2 \xrightarrow{{{k_2}}} N_2O + H_2O\,$    (slow)

$(iii)$  $N_2O + H_2 \to N_2 + H_2O\,$   (fast)

then what will be the rate law of this reaction ?

For the following parallel chain reaction. What will be that value of overall half-life of $A$ in minutes ?

Given that  $\left[ {\frac{{{{\left[ B \right]}_t}}}{{{{[C]}_t}}} = \frac{{16}}{9}} \right]$

$A\,\xrightarrow{{{K_1}\, = \,2\, \times \,{{10}^{^{ - 3}\,}}{S^{ - 1}}}}4B$

$A\to C$

$A + 2B \to C$, the rate equation for this reaction is given as Rate $= K[A][B]$ . If the concentration of $A$ is kept the same but that of $B$ is doubled what will happen to the rate it self ?

The rate of the reaction becomes twice when the concentration of reactant becomes $8$ times then the order of the reaction is

For any reaction, if we plot a graph between time '$t$' and $\log (a - x)$, a simple line is obtained. The order of reaction is

The dimension of rate constant of a second order reaction involves