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Chemistry Question on Chemical Kinetics

The half-life for a zero order reaction having 0.02 M0.02\, M initial concentration of reactant is 100 s100\, s. The rate constant (in mol L−1s−1)mol \,L^{-1} s^{-1}) for the reaction is

A

1.0×10−41.0 \times 10^{-4}

B

2.0×10−42.0 \times 10^{-4}

C

2.0×10−32.0 \times 10^{-3}

D

1.0×10−21.0\times 10^{-2}

Answer

1.0×10−41.0 \times 10^{-4}

Explanation

Solution

(t1/2)zero=[A]02K(t_{1/2})_{\text{zero}}=\frac{[A]_{0}}{2K} 100S=0.02M2K100S=\frac{0.02M}{2K} K=0.02M2×100K=\frac{0.02M}{2 \times 100} =1×10−4mol L−1 s−1=1 \times 10^{-4}mol\,L^{-1}\,s^{-1}