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Arrhenius Equation

What is the a...

Question

What is the activation energy for the decomposition of $N_{2} O_{5}$ as, $N_{2} O_{5} \to$ 2 $N O_{2} + \frac{1}{2} O_{2}$ . if the values of the rate constants are $3.45 \times 10^{- 5}$ and $6.9 \times 10^{- 3}$ at $27^{0} C$ and $67^{0} C$ respectively?

A

112.5 kJ

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B

200 kJ

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C

149.5 kJ

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D

11.25 kJ

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Solution

The correct option is D 112.5 kJ
The expression for the relationship between the rate constants at two different temperatures is as shown below.
$log \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 R} \frac{(T_{2} - T_{1})}{T_{1} T_{2}}$

Substitute values in the above expression.
$l o g \frac{6.9 \times 10^{- 3}}{3.45 \times 10^{- 5}} = \frac{E_{a}}{2.303 \times 8.314} \frac{340 - 300}{300 \times 340}$

$E_{a} = 112.5 k J$ .

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Similar questions

Q. If the rate of decomposition of

N_{2} O_{5}

during a certain time internal is

2.4 \times 10^{- 4} m o l L^{- 1} m i n^{- 1}

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

What is the rate of formation of

N O_{2}

O_{2} m o l L^{- 1} m i n^{- 1}

Q. For decomposition of

N_{2} O_{5}

, rate constant were determined at two different temperature. At

27^{\circ} C,

rate constant was

2 \times 10^{- 4} {sec}^{- 1}

47^{\circ} C

the rate constant is

6 \times 10^{- 4} {sec}^{- 1}

.
Then identify the correct statement(s).
(Given

l n 3 = 1.1

)

Q. If rate constants for decomposition of

N_{2} O_{5}

N O_{2}

and formation of

O_{2}

K_{1}, K_{2}

K_{3}

respectively, then:

Q. The container of

2

litrer contains

4

N_{2} O_{5}

. On heating to

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

undergoes complete dissociation to

N O_{2}

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}

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

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