The rate constant for the reaction N2O5 → 4NO2 + O2 is 3.0 × 10−5 s−1. If the rate of reaction is 2.

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The rate constant for the reaction N2O5 → 4NO2 + O2 is 3.0 × 10−5 s−1. If the rate of reaction is 2.4 × 10−5 mol litre−1 s−1, then the concentration of N2O5 (in mole litre−1) is

Accepted Answer

$r = K\left\lbrack N_{2}O_{5} ightbrack$$\Rightarrow \left\lbrack N_{2}O_{5} ightbrack = \frac{r}{K} = \frac{2.4 	imes 10^{- 5}	ext{ M}	ext{s}^{- 1}}{3.0 	imes 10^{- 5}	ext{ }	ext{s}^{- 1}} = 0.8	ext{ M}$

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