If the concentration of a first-order reaction is increased by $x$ times,then the rate constant $(k)$ becomes

The hydrolysis of an ester is catalyzed by dilute acids $A$ and $B$. The rate constants for the two processes are $K_A$ and $K_B$ respectively. If $K_A > K_B$,which of the following statements is correct?

The mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. The rate of reaction doubles if:

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:

The rate of reaction between $A$ and $B$ increases by a factor of $100$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is