The rate law for the decomposition of hydrogen iodide is $-\frac{d[HI]}{dt}=k[HI]^2$. The units of rate constant $k$ are

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

$A + B \rightarrow \text{product}$. The rate of this reaction is given by $v = K[A]^2[B]^0$. What is the change in the rate of reaction when the concentration of $A$ is doubled and the concentration of $B$ is doubled?