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Chemistry Question on Chemical Kinetics

The decomposition of      N2O5(g)⟶ NO2(g)+NO3(g) \, \, \, \, \, N_2 O_5 (g) \longrightarrow \, NO_2 (g) + NO_3 (g) proceeds as a first order reaction with a half-life period of 30 s30 \,s at a certain temperature. If the initial concentration [N2O5]=0.4 M[N_2 O_5] = 0.4 \, M, what is the rate constant of the reaction?

A

0.00924 s−10.00924\,s^{-1}

B

0.0231 s−10.0231\,s^{-1}

C

75 s−175\,s^{-1}

D

12 s−112\,s^{-1}

Answer

0.0231 s−10.0231\,s^{-1}

Explanation

Solution

For a first order reaction
\hspace25mm k = \frac{0.693}{t_{1/2}} = \frac{0.693}{30} = 0.0231 s^{-1}