The rate constant of the reaction, $2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}$ at $300 K$ is $3 \times 10^{- 5} s^{- 1}$ . If the rate of the reaction at the same temperature is $2.4 \times 10^{- 5}$ $m o l$ ${d m}^{- 3} s^{- 1}$ , then the molar concentration of $N_{2} O_{5}$ is:

0.4 M

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0.8 M

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0.04 M

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0.08 M

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0.6 M

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Solution

The correct option is B $0.8 M$
Given that,
Rate constant, $k$ $= 3 \times 10^{- 5} s^{- 1}$ which indicates that reaction is of first order. ( $∵$ unit is $s^{- 1}$ )
$∴$ Rate of reaction $r = k {[C]}^{1}$

$∴ [C] = \frac{r}{k}$
$∴ [C] = \frac{2.4 \times 10^{- 5}}{3.0 \times 10^{- 5}} = 0.8 M$

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Similar questions

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

3 \times 10^{- 5} s^{- 1}

2.4 \times 10^{- 5} M s^{- 1}

N_{2} O_{5}

^{- 1}

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

1.02 \times 10^{- 4}

3.4 \times 10^{- 5} s^{- 1}

N_{2} O_{5}

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

Expt. No.	$[N_{2} O_{5}]$ $(m o l L^{- 1})$	Rate of disappearance of $N_{2} O_{5}$ $(m o l L^{- 1} {m i n}^{- 1})$
$1.$	$1.13 \times 10^{- 2}$	$34 \times 10^{- 5}$
$2.$	$0.84 \times 10^{- 2}$	$25 \times 10^{- 5}$
$3.$	$0.62 \times 10^{- 2}$	$18 \times 10^{- 5}$