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Standard XII

Chemistry

Rate Constant

At 2500C, t...

Question

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:

0.693 / 5.7

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0.693 \times 3.7

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5.7 / 0.693

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None

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Solution

The correct option is D $0.693 / 5.7$
Decomposition of $N_{2} O_{5}$ is a 1st Order Reaction.

$t_{1 / 2} = \frac{0.693}{k}$
$k = \frac{0.693}{5.7}$

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Similar questions

Q. At

373

k the half-life period for the thermal decomposition of

N_{2} O_{5}

4.6

sec and is independent of the initial pressure of

N_{2} O_{5}

. Calculate the specific rate constant of this temperature.

Q. 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}

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}

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.

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)

The first-order rate constant for the decomposition of $N_{2} O_{5}$ is $6.2 \times 10^{- 4} s^{- 1}$ . The half-life for this decomposition is___?

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At 2500C, the half life for decomposition of N2O5 is 5.7 hr and is independent of initial pressure of N2O5. The specific rate constant is:

The correct option is D 0.693/5.7Decomposition of N2O5 is a 1st Order Reaction.t1/2=0.693kk=0.6935.7

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:

The correct option is D $0.693 / 5.7$
Decomposition of $N_{2} O_{5}$ is a 1st Order Reaction.

$t_{1 / 2} = \frac{0.693}{k}$
$k = \frac{0.693}{5.7}$