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 $100s^{-1}100\; \backslash ,s^\{-1\}$ 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 $C_{0}C\_0$ 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 $R=k[A{]}^n\times [B{]}^{m}R\; =\; k\; [A]^n\; \backslash times\; [B]\; ^m$ 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 $\to \backslash rightarrow$ 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, $C{l}_2+2I^{-}\to 2C{I}^{-}+I_{2}Cl\_2\; +\; 2I^-\; \backslash rightarrow\; 2CI^-+\; I\_2$ , the initial concentration of $I^{-}I^-$ was $0.2mol{L}^{-1}0.2\; \backslash \; mol\; \backslash \; L^\{-1\}$ and the concentration after 20 minutes was $0.18mol{L}^{-1}0.18\; \backslash \; mol\; \backslash \; L^\{-1\}$ . Then the rate of formation of $I_{2}I\_2$ in mol $L^{-1}L^\{-1\}$ $mi{n}^{-1}min^\{-1\}$ will be