$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?

Write the differential rate expression for the following reaction and determine its order of reaction:
$H_{2}O_{2} + I^{-} \rightarrow H_{2}O + IO^{-}$
$H_{2}O_{2} + IO^{-} \rightarrow H_{2}O + I^{-} + O_{2}$

The rate constant of which of the following reactions is independent of the concentration of the reactants?

The rate constant is the same for $3$ reactions of order $I, II$,and $III$,respectively,with the unit of concentration being in moles per litre. If the concentration of the reactant is unity,the rates of reaction $R_1, R_2, R_3$ will be:

Fill in the blanks:
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$

For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?