In a first order reaction the concentration of reactant decreases from $800 m o l / {d m}^{3}$ to $50 m o l / {d m}^{3}$ in $2 \times 10^{2} s$ . The rate constant of reaction in $s^{- 1}$ is:

2 \times 10^{4}

3.45 \times 10^{- 5}

1.386 \times 10^{- 2}

2 \times 10^{- 4}

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In a first order reaction the concentration of reactant decreases from 800mol/dm3 to 50mol/dm3 in 2×102s. The rate constant of reaction in s−1 is:

In a first order reaction the concentration of reactant decreases from $800 m o l / {d m}^{3}$ to $50 m o l / {d m}^{3}$ in $2 \times 10^{2} s$ . The rate constant of reaction in $s^{- 1}$ is: