For a second-order reaction where the initial concentrations of both reactants are equal,it takes $3000 \ s$ for the reaction to be $60\%$ complete. How much time (in $s$) will it take for the reaction to be $20\%$ complete?

For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.

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?

For a certain chemical reaction $X \rightarrow Y$,the rate of formation of the product is plotted against time as shown in the figure. The number of correct statement$(s)$ from the following is $.......$.
$A$. Overall order of this reaction is one
$B$. Order of this reaction cannot be determined
$C$. In region-$I$ and $III$,the reaction is of first and zero order respectively
$D$. In region-$II$,the reaction is of first order
$E$. In region-$II$,the order of reaction is in the range of $0.1$ to $0.9$.

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

If the value of the rate constant $K = 2.3 \times 10^{-5} \ L \ mol^{-1} \ s^{-1}$,then identify the reaction order: