The decomposition of in chloroform was followed by measuring the volume of gas…

CHEMISTRY · Single correct · CBSE · Chemistry · Chemical Kinetics · Chemical Kinetics

Problem

The decomposition of

\mathrm{N_2O_5}

in chloroform was followed by measuring the volume of

\mathrm{O_2}

gas evolved:

2\mathrm{N_2O_5}(\mathrm{CCl_4})\rightarrow2\mathrm{N_2O_4}(\mathrm{CCl_4})+\mathrm{O_2}(g).

The maximum volume of

\mathrm{O_2}

gas obtained was

100\,\text{cm}^3

. In

500\,\text{min}

90\,\text{cm}^3

\mathrm{O_2}

was evolved. The first-order rate constant, in

\text{min}^{-1}

, for the disappearance of

\mathrm{N_2O_5}

is: (a)

\frac{2.303}{500}

(b)

\frac{2.303}{500}\log\frac{100}{90}

(c)

\frac{2.303}{500}\log\frac{90}{100}

(d)

\frac{100}{10\times500}