For the reaction $H_{2(g)} + Br_{2(g)} \to 2HBr_{(g)}$,the experimental data suggest,$\text{rate} = K[H_2][Br_2]^{1/2}$. The molecularity and order of the reaction are respectively:

For the reaction system $2NO_{(g)} + O_{2(g)} \to 2NO_{2(g)}$,the volume is suddenly reduced to half its initial value by increasing the pressure. If the reaction is of first order with respect to $O_2$ and second order with respect to $NO$,the rate of reaction will:

The rate of the simple reaction,$2NO + O_2 \to 2NO_2$,when the volume of the reaction vessel is doubled:

Which of the following statements is correct?

The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

Total order of reaction $X + Y \rightarrow XY$ is $3$. The order of reaction with respect to $X$ is $2$. State the differential rate equation for the reaction.