For a first order reaction involving decomposition of N 2 O 5- the following information is available - 2 N 2 O 5 g - 4NO 2 g - O 2 g Rate - k - N 2 O 5 - N 2 O 5g - 2NO 2g - 1 - 2 O 2g Rate - k - - N 2 O 5 -Which of the following expressions is true -

The correct option is B k > k ^' (I) 2N_2O_5(g) → 4NO_2(g)+O_2(g) Rate =K[N_2O_5] (II) N_2O_5(g) → 2NO_2(g)+12O_2(g) Rate =K'[N_2O_5 ...

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Byju's Answer

Standard XII

Chemistry

First Order Reaction

For a first o...

Question

For a first order reaction involving decomposition of $N_{2} O_{5}$ , the following information is available :
$2 N_{2} O_{5} (g)$ $\to$ ${4 N O}_{2} (g)$ + $O_{2} (g)$ Rate = k $[N_{2} O_{5}]$
$N_{2} O_{5}$ (g) $\to$ ${2 N O}_{2}$ (g) + $\frac{1}{2} O_{2}$ (g) Rate = $k^{'}$ $[N_{2} O_{5}]$ ,
Which of the following expressions is true ?

k =

k^{'}

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k^{'}

= 2k

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k^{'}

1 / 2 k

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k >

k^{'}

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Solution

The correct option is B k > $k^{'}$
(I) $2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g)$ Rate $= K [N_{2} O_{5}]$
(II) $N_{2} O_{5} (g) \to 2 N O_{2} (g) + \frac{1}{2} O_{2} (g)$ Rate $= K^{'} [N_{2} O_{5}]$
we know that
$(I)$ $K = \frac{[N O_{2}] [O_{2}]}{[N_{2} O_{5}]^{2}}$
$(I I)$ $K^{'} = \frac{[N O_{2}]^{2} [O_{2}]^{1 / 2}}{N_{2} O_{5}}$
Squaring both side
$K^{' 2} = \frac{[N O_{2}]^{4} [O_{2}]}{[N_{2} O_{5}]^{5}}$
$K^{' 2} = K$
$K^{'} = \sqrt{K}$
Ans $k > k^{'}$

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Similar questions

Q. The rate of the reaction

2 N_{2} O_{5} ⟶ 4 N O_{2} + O_{2}

can be written in three ways:

\frac{- d [N_{2} O_{5}]}{d t} = k [N_{2} O_{5}]

\frac{d [N O_{2}]}{d t} = k^{'} [N_{2} O_{5}]

\frac{d [O_{2}]}{d t} = k^{''} [N_{2} O_{5}]

The relationship between

k

and

k^{'}

and between

k

and

k^{''}

are :

Q. The rate constant

k

, for the reaction

N_{2} O_{5} (g) ⟶ 2 {N O}_{2} (g) + \frac{1}{2} O_{2} (g)

1.3 \times 10^{- 2} s^{- 1}

. Which equation given below describes the change of

[N_{2} O_{5}]

with time?

{[N_{2} O_{5}]}_{0}

and

{[N_{2} O_{5}]}_{t}

correspond to concentration of

N_{2} O_{5}

initially and at time

t

Q. The initial concentration of

N_{2} O_{5}

in the first order reaction

N_{2} O_{5 (g)} ⟶ {2 N O}_{2 (g)} + \frac{1}{2} O_{2 (g)}

was 1

1.24 \times 10^{- 2} m o l L^{- 1}

at 318 K. The concentration of

N_{2} O_{5}

after 60 minutes was

{0.20 \times 10}^{- 2} m o l L^{- 1}

. Calculate the rate constant of the reaction at 318 K.

Q. The rate constant for the reaction,

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

, is

2.3 \times 10^{- 2} {s e c}^{- 1}

. Which equation given below describes the change of

[N_{2} O_{5}]

with time,

{[N_{2} O_{5}]}_{0}

and

{[N_{2} O_{5}]}_{t}

corresponds to concentration of

N_{2} O_{5}

initially and time

t

respectively?

Q. What is the ratio between the rate of decomposition of

N_{2} O_{5}

to rate of formation of

N O_{2}

2 N_{2} O_{5 (g)} ⟶ 4 N O_{2 (g)} + O_{2 (g)}

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For a first order reaction involving decomposition of N2O5, the following information is available :2N2O5(g) → 4NO2(g) + O2(g) Rate = k [N2O5]N2O5(g) → 2NO2(g) + 12O2(g) Rate = k′ [N2O5],Which of the following expressions is true ?

The correct option is B k > k′(I) 2N2O5(g)→4NO2(g)+O2(g) Rate =K[N2O5](II) N2O5(g)→2NO2(g)+12O2(g) Rate =K′[N2O5]we know that (I) K=[NO2][O2][N2O5]2(II) K′=[NO2]2[O2]1/2N2O5Squaring both sideK′2=[NO2]4[O2][N2O5]5K′2=KK′=√KAns k>k′