The rate constant for a zero order reaction is $2 \times 10^{-2} \ mol \ L^{-1} s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,the initial concentration must have been $:-$ (in $M$)

The half-life of a zero order reaction $A \rightarrow \text{products}$ is $0.5 \ hr$. The initial concentration of $A$ is $4 \ mol \ L^{-1}$. How much time (in $hr$) does it take for its concentration to come from $2.0 \ mol \ L^{-1}$ to $1.0 \ mol \ L^{-1}$?

For a zero order reaction,$A \longrightarrow \text{product}$,the concentration of $A$ decreases from $1.2 \ mol \ dm^{-3}$ to $0.4 \ mol \ dm^{-3}$ in $240 \ s$. What is the rate constant of the reaction?

The rate constant of the reaction $A \rightarrow B$ is $0.6 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}.$ If the concentration of $A$ is $5 \, M,$ then the concentration of $B$ after $20$ minutes is ......... $M.$

The plot of concentration of a reactant versus time for a chemical reaction is shown below. The order of this reaction with respect to the reactant is

For a given reaction,the half-life $t_{1/2}$ varies with different initial concentrations $a$. If $t_{1/2} \propto a$ is constant,then the order of the reaction will be .......