The acidic hydrolysis of an ester is a .......

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

Rate of the reaction $A + B \rightarrow \text{product}$ is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ and rate law is $r = k[A][B]^2$. What is the rate constant of the reaction if $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$?

Acid catalysed hydrolysis of ethyl acetate follows a pseudo-first order kinetics with respect to ester. If the reaction is carried out with large excess of ester, the order with respect to ester will be

$(a)$ Write the general reaction and derive the units of the rate constant. $(b)$ Based on that,write the rate constant units for zero,first,and $2^{nd}$ order reactions.

If a reaction has the experimental rate expression $\text{rate} = K [A]^2[B]$,what happens to the reaction rate if the concentration of $A$ is doubled and the concentration of $B$ is halved?