The container of 2 litrer contains 4 mole of N2O5- On heating to 100-C- N2O5 undergoes complete dissociation to NO2 and O2- Select the correct answers if rate constant for decomposition of N2O5 is 6-2- 10-4sec-1-1- The mole ratio before and after dissociation is 4 - 22- Half life of N2O5 is 1117 sec and it is independent of concentration-3- Time required to complete 40

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Standard VII

Chemistry

Half Life

The container...

Question

The container of $2$ litrer contains $4$ mole of $N_{2} O_{5}$ . On heating to $100^{\circ} C, N_{2} O_{5}$ undergoes complete dissociation to $N O_{2}$ and $O_{2}$ . Select the correct answers if rate constant for decomposition of $N_{2} O_{5}$ is $6.2 \times 10^{- 4} s e c^{- 1}$ .
1. The mole ratio before and after dissociation is $4 : 2$
2. Half life of $N_{2} O_{5}$ is $1117 s e c$ and it is independent of concentration.
3. Time required to complete $40$ % of reaction is $824 s e c$ .
4. If volume of container is doubled, the initial rate of decomposition becomes half of the initial rate.

1, 3, 4

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1, 2, 3, 4

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3, 4

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2, 3, 4

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Solution

The correct option is C $3, 4$
Because reaction is first order
$ϑ = k [A]$
$A = A_{0} e^{- k t}$
for which
$t_{40} = 824$ sec
if $v_{f} = 2 V_{i} \Rightarrow C_{f} = \frac{C_{i}}{2} \Rightarrow ϑ_{f} = \frac{ϑ_{i}}{2}$

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Similar questions

Q. The container of 2 litre contains 4 mole of

N_{2} O_{5}

. On heating to

100^{o} C, N_{2} O_{5}

undergoes complete dissociation to

N O_{2}

and

O_{2}

. Select the correct answers if rate constant for decomposition of

N_{2} O_{5}

6.2 \times 10^{- 4} s e c^{- 1}

.
1. The mole ratio before and after dissociation is 4:2.
2. The half-life of

N_{2} O_{5}

is 1117.7 sec and it is independent of temperature.
3. The time required to complete 40% of reaction is 824 sec.
4. If the volume of the container is doubled, the rate of decomposition becomes half of the initial rate

Q. A container of

2 l i t r e

capacity contains 4 moles of

N_{2} O_{5}

. On heating to

100^{\circ} C, N_{2} O_{5}

undergoes dissociation to give

N O_{2}

and

O_{2}

. Select the correct answer among the following if the rate constant for decomposition of

N_{2} O_{5}

6.3 \times 10^{- 4} s e c^{- 1} . (l n 2 = 0.693)

Q. For the reaction

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

, if the initial concentration of

N_{2} O_{5}

7.2 m o l L^{- 1}

and after

20

minutes,

[N O_{2}]

becomes

2.4 m o l L^{- 1}

, then what will be rate of decomposition of

N_{2} O_{5}

m o l L^{- 1} m i n^{- 1}

Q. At

250^{0} C

, the half life for decomposition of

N_{2} O_{5}

is 5.7 hr and is independent of initial pressure of

N_{2} O_{5}

. The specific rate constant is:

Q. The decomposition of

N_{2} O_{5}

dissolved in carbontetrachloride occurs as follows.

N_{2} O_{5_{(S o l u t i o n)}} ⇌ 2 N O_{2_{(S o l u t i o n)}} + \frac{1}{2} O_{2 (g)}

.
This reaction is of first order and its rate constant is

5.0 \times 10^{- 4} s e c^{- 1}

. If initial concentration of

N_{2} O_{5}

for this reaction is

0.50 m o l e l i t r e^{- 1}

, then
a) What will be the initial reaction rate?
b) What will be half life period of this reaction?
c) What will be the concentrations of

N_{2} O_{5}

and

N O_{2}

at the end of

50

minutes after the starting of reaction?

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The correct option is C 3,4Because reaction is first orderϑ=k[A]A=A0e−ktfor whicht40=824secifvf=2Vi⇒Cf=Ci2⇒ϑf=ϑi2

The correct option is C $3, 4$
Because reaction is first order
$ϑ = k [A]$
$A = A_{0} e^{- k t}$
for which
$t_{40} = 824$ sec
if $v_{f} = 2 V_{i} \Rightarrow C_{f} = \frac{C_{i}}{2} \Rightarrow ϑ_{f} = \frac{ϑ_{i}}{2}$