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The decomposition of N2O5 according to the equation,
N2O5(g) → 4NO2(g) + O2(g)
Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.
- a)5.2 × 10-3 min-1
- b)2.26 × 10-3 min-1
- c)5.2 × 10-6 min-1
- d)2.20 × 10-3 min-1
Correct answer is option 'A'. Can you explain this answer?
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The decomposition of N2O5 according to the equation,N2O5(g) U...
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The decomposition of N2O5 according to the equation,N2O5(g) U...
Given:
N2O5(g) → 4NO2(g) + O2(g)
The reaction is first order.
Total pressure after 30 minutes = 284.4 mmHg
Total pressure on completion = 584.5 mmHg
To find: Rate constant of the reaction.
Solution:
We know that the reaction is first order, so the rate law can be written as:
Rate = k[N2O5]
We can use the following equation to relate the pressure to the concentration of N2O5:
P = (nRT/V) = (m/M)RT/V = (cRT) / M
where,
P = pressure
n = number of moles
R = gas constant
V = volume
m = mass
M = molar mass
c = concentration
At time t = 0, the pressure of N2O5 is P0.
After 30 minutes, the pressure of N2O5 is given by:
P1 = (cRT/ M) = (P0 - 4x)RT/M
where,
x = pressure of NO2 at time t = 30 minutes
On completion of the reaction, the pressure of N2O5 is zero, so the pressure of NO2 is equal to the total pressure.
Therefore, the pressure of NO2 at completion is:
P2 = (cRT/M) = (584.5 - x)RT/M
The rate constant can be calculated using the following equation:
k = (2.303/t) log (P0/Pt)
where,
t = time taken for the reaction to complete
Pt = pressure of N2O5 at time t
2.303 = conversion factor
Substituting the values, we get:
k = (2.303/30) log (P0/584.5)
k = 5.2 x 10^-3 min^-1
Therefore, the correct answer is option A.
N2O5(g) → 4NO2(g) + O2(g)
The reaction is first order.
Total pressure after 30 minutes = 284.4 mmHg
Total pressure on completion = 584.5 mmHg
To find: Rate constant of the reaction.
Solution:
We know that the reaction is first order, so the rate law can be written as:
Rate = k[N2O5]
We can use the following equation to relate the pressure to the concentration of N2O5:
P = (nRT/V) = (m/M)RT/V = (cRT) / M
where,
P = pressure
n = number of moles
R = gas constant
V = volume
m = mass
M = molar mass
c = concentration
At time t = 0, the pressure of N2O5 is P0.
After 30 minutes, the pressure of N2O5 is given by:
P1 = (cRT/ M) = (P0 - 4x)RT/M
where,
x = pressure of NO2 at time t = 30 minutes
On completion of the reaction, the pressure of N2O5 is zero, so the pressure of NO2 is equal to the total pressure.
Therefore, the pressure of NO2 at completion is:
P2 = (cRT/M) = (584.5 - x)RT/M
The rate constant can be calculated using the following equation:
k = (2.303/t) log (P0/Pt)
where,
t = time taken for the reaction to complete
Pt = pressure of N2O5 at time t
2.303 = conversion factor
Substituting the values, we get:
k = (2.303/30) log (P0/584.5)
k = 5.2 x 10^-3 min^-1
Therefore, the correct answer is option A.
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The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer?
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The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer?.
The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer?.
Solutions for The decomposition of N2O5 according to the equation,N2O5(g) → 4NO2(g) + O2(g)Is a first order reaction. After 30 minutes from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.4 mmHg and on completion, the total pressure is 584.5 mmHg. Calculate the Rate constant of the reaction.a)5.2 × 10-3min-1b)2.26 × 10-3min-1c)5.2 × 10-6min-1d)2.20× 10-3min-1Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for IIT JAM.
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