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The decomposition of N2O5 according to following reaction is first order
2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction.
2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction.
- a)6 × 1013
- b)6 × 103
- c)6 × 10-3
- d)6 × 10-13
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
The decomposition of N2O5 according to following reaction is first ord...
For the given reaction:
2N2O5(g)→4NO2(g)+O2(g)
2N2O5(g)→4NO2(g)+O2(g)
a 0 0 -------- initial time (t=0)
a−X 2X X/2 ------- after time (t=30 min)
a−X 2X X/2 ------- after time (t=30 min)
0 2a a/2 ----- after complete reaction
∵ No. of mole at any time ∝ pressure developed at that time
∵ No. of mole at any time ∝ pressure developed at that time
∴a ∝ P0 at t=0 -----1
a+(3X/2)∝284.5 at t=30 ------ 2
(5a/2)∝584.5 at t=completely reacted ------ 3
a+(3X/2)∝284.5 at t=30 ------ 2
(5a/2)∝584.5 at t=completely reacted ------ 3
From 1 and 3 equation, we get
∴a ∝ 233.8 ----------------------- 4
Substituting 4 in 2 equation we get
X∝33.8 --------------------------------- 5
Now,
∴ K = 2.303/t log a/(a−X)
∴ K = 2.303/30 log233.8/200
∴ K = 2.303/t log a/(a−X)
∴ K = 2.303/30 log233.8/200
= 5.206 × 10-3min-1
Most Upvoted Answer
The decomposition of N2O5 according to following reaction is first ord...
For the given reaction:
2N2O5(g)→4NO2(g)+O2(g)
2N2O5(g)→4NO2(g)+O2(g)
a 0 0 -------- initial time (t=0)
a−X 2X X/2 ------- after time (t=30 min)
a−X 2X X/2 ------- after time (t=30 min)
0 2a a/2 ----- after complete reaction
∵ No. of mole at any time ∝ pressure developed at that time
∵ No. of mole at any time ∝ pressure developed at that time
∴a ∝ P0 at t=0 -----1
a+(3X/2)∝284.5 at t=30 ------ 2
(5a/2)∝584.5 at t=completely reacted ------ 3
a+(3X/2)∝284.5 at t=30 ------ 2
(5a/2)∝584.5 at t=completely reacted ------ 3
From 1 and 3 equation, we get
∴a ∝ 233.8 ----------------------- 4
Substituting 4 in 2 equation we get
X∝33.8 --------------------------------- 5
Now,
∴ K = 2.303/t log a/(a−X)
∴ K = 2.303/30 log233.8/200
∴ K = 2.303/t log a/(a−X)
∴ K = 2.303/30 log233.8/200
= 5.206 × 10-3min-1
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Community Answer
The decomposition of N2O5 according to following reaction is first ord...
→ 4 NO2 + O2
If the decomposition of N2O5 is first order, it means that the rate of the reaction is directly proportional to the concentration of N2O5 raised to the power of 1.
Mathematically, the rate equation for a first-order reaction can be written as follows:
rate = k[N2O5]^1
Where:
- rate is the rate of the reaction
- k is the rate constant
- [N2O5] is the concentration of N2O5
Therefore, for the given reaction:
rate = k[N2O5]^1
If the decomposition of N2O5 is first order, it means that the rate of the reaction is directly proportional to the concentration of N2O5 raised to the power of 1.
Mathematically, the rate equation for a first-order reaction can be written as follows:
rate = k[N2O5]^1
Where:
- rate is the rate of the reaction
- k is the rate constant
- [N2O5] is the concentration of N2O5
Therefore, for the given reaction:
rate = k[N2O5]^1
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The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer?
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The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer?.
The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer?.
Solutions for The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
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ample number of questions to practice The decomposition of N2O5 according to following reaction is first order 2 N2O5 → 4 NO2(g) + O2 (g). After 30 minutes from the start of decomposition in a closed vessel the total pressure developed is found to be 250 mm of Hg and on complete decomposition the total pressure is 500 mm of Hg. Calculate rate constant of the reaction. a)6 × 1013 b)6 × 103 c)6 × 10-3 d)6 × 10-13Correct answer is option 'C'. Can you explain this answer? tests, examples and also practice Chemistry tests.
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