Chemical Kinetics Quiz 3

Time required to complete 90% of the first order reaction is

The half-life of a first order reaction is 30 min and the initial concentration of the reactant is 0.1M. If the initial concentration of reactant is doubled, then the half-life of the reaction will be

The rate constant for a first order reaction is $100 \,s^{-1}$ the time required for completion of 50% of reaction is-

The slope of the straight line obtained by plotting rate versus concentration of reactant for a first order reaction is

If $C_0$ and C are the concentrations of a reactant initially and after time t then, for a first order reaction

When half-life period of a zero order reaction is plotted against concentration of the reactant at constant temperature, the graph obtained is

The rate of a reaction between A and B is $R = k [A]^n \times [B] ^m$ On doubling the concentration of A and halving the concentration of B, the ratio of the new rate to the earlier rate of the reaction will be

The rate of the first order reaction A $\rightarrow$ products is 0.01 M/s, when reactant concentration is 0.2 M. The rate constant for the reaction will be

The rate constant of a reaction

For the reaction, $Cl_2 + 2I^- \rightarrow 2CI^-+ I_2$ , the initial concentration of $I^-$ was $0.2 \ mol \ L^{-1}$ and the concentration after 20 minutes was $0.18 \ mol \ L^{-1}$ . Then the rate of formation of $I_2$ in mol $L^{-1}$ $min^{-1}$ will be