For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will:

$A$ complex reaction takes place in $2$ steps:
$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)
$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)
Identify the reaction intermediate.

For the reaction: $2 A + B \rightarrow A_2 B$,the rate $= k[A][B]^2$ with $k = 2.0 \times 10^{-6} \ mol^{-2} \ L^2 \ s^{-1}$. Calculate the initial rate of the reaction when $[A] = 0.1 \ mol \ L^{-1}$ and $[B] = 0.2 \ mol \ L^{-1}$. Calculate the rate of reaction after $[A]$ is reduced to $0.06 \ mol \ L^{-1}$.

The reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism $A_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2A$ (fast),$A + B_2 \xrightarrow{k_2} AB + B$ (slow),$A + B \rightarrow AB$ (fast). The overall order of the reaction is:

The three experimental data for determining the differential rate of reaction $Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$ at $310 \ K$ temperature are provided. $(a)$ Derive the differential rate of reaction. $(b)$ Calculate the order of reaction. $(c)$ Calculate the value of the rate constant.

For the reaction $2A + B \rightarrow \text{Product}$,the half-life remains unchanged when the concentration of $A$ is doubled. When the concentration of $B$ is doubled,the rate of reaction increases by a factor of $2$. What is the unit of the rate constant for this reaction?