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Zero Order Reaction

The decomposi...

Question

The decomposition of $N_{2} O_{5}$ in ${C C l}_{4}$ solution at 320 K takes place as ${2 N}_{2} O_{5} \to {4 N O}_{2} + O_{2}$ ; On the bases of given data order and the rate constant of the reaction is :
$\begin{matrix} T i m e i n m i n u t e s & 10 & 15 & 20 & 25 & \infty V o l u m e o f O_{2} & 6.30 & 8.95 & 11.40 & 13.50 & 34.75 \end{matrix}$
$e v o l v e d (i n m L)$

1, 0.198

{m i n}^{- 1}

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3 / 2, 0.0198

M^{- 1 / 2}

{m i n}^{- 1}

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0, 0.0198

M

{m i n}^{- 1}

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1, 0.0198

{m i n}^{- 1}

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Solution

The correct option is D $1, 0.0198$ ${m i n}^{- 1}$
Hence, Option D is correct.

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Similar questions

N_{2} O_{5}

N_{2} O_{5} ⟶ 2 N O_{2} + \frac{1}{2} O_{2}

N_{2} O_{5}

1.8 \times 10^{- 3}

m o l

{l i t r e}^{- 1}

{m i n}^{- 1}

N O_{2}

O_{2}

N_{2} O_{5}

N_{2} O_{5} \to N_{2} O_{4} + \frac{1}{2} O_{2}

O_{2}

[G i v e n 2.303 log (\frac{4}{3}) = 0.28]

N_{2} O_{5}

C C l_{4}

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

Time in minutes	10	15	20	25	$\infty$
The volume of $O_{2}$ evolved (in mL)	6.30	8.95	11.40	13.50	34.75

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 $N_{2} O_{5}$ $(m o l L^{- 1} {m i n}^{- 1})$
$1.$	$1.13 \times 10^{- 2}$	$34 \times 10^{- 5}$
$2.$	$0.84 \times 10^{- 2}$	$25 \times 10^{- 5}$
$3.$	$0.62 \times 10^{- 2}$	$18 \times 10^{- 5}$

N_{2} O_{5} [2 N_{2} O_{5} ⟶ {4 N O}_{2} + O_{2}]

$t / s$	0	400	800	1200	1600	2000	2400	2800	3200
$10^{- 2} \times [N_{2} O_{5}] / m o l L^{- 1}$	1.63	1.36	1.14	0.93	0.78	0.64	0.53	0.43	0.35

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