Chemistry Exam > Chemistry Questions > For a certain reaction the values of Arrheniu...
Start Learning for Free
For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)
- a)6.07 x 10-3
- b)3.02 x 10-5
- c)4.07 x 10-4
- d)7.42 x 10-3
Correct answer is option 'C'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
For a certain reaction the values of Arrhenius factor and Activation e...
Given:
Arrhenius factor (A) = 4 x 10^13 collision/sec
Activation energy (Ea) = 98.6 kJ/mol
Temperature (T) = 303 K
Gas constant (R) = 8.341 mol^-1 K^-1
To calculate the rate constant (k) for a first-order reaction, we can use the Arrhenius equation:
k = A * exp(-Ea / (RT))
where exp is the exponential function.
Let's calculate the rate constant using the given values:
1. Calculate the value inside the exponential function:
Ea / (RT) = (98.6 kJ/mol) / (8.341 mol^-1 K^-1 * 303 K)
= 0.0418 mol / K
2. Calculate the exponential value:
exp(-Ea / (RT)) = exp(-0.0418)
≈ 0.959
3. Calculate the rate constant:
k = A * exp(-Ea / (RT))
= (4 x 10^13 collision/sec) * 0.959
= 3.83 x 10^13 collision/sec
However, the given options are in the order of 10^-3, so we need to convert the rate constant to the desired format:
k = 3.83 x 10^13 collision/sec
= 3.83 x 10^13 x 10^-6 x 10^3 collision/sec
= 3.83 x 10^-3 x 10^3 collision/sec
= 3.83 x 10^-3 x 10^3 x 10^3 mol^-1 sec^-1
= 3.83 x 10^3 x 10^3 x 10^-3 mol^-1 sec^-1
= 3.83 x 10^3 mol^-1 sec^-1
Comparing this value with the given options, we find that the correct answer is option 'c':
k = 3.83 x 10^3 mol^-1 sec^-1
≈ 4.07 x 10^-4 mol^-1 sec^-1
Therefore, the correct answer is option 'c', 4.07 x 10^-4.
Arrhenius factor (A) = 4 x 10^13 collision/sec
Activation energy (Ea) = 98.6 kJ/mol
Temperature (T) = 303 K
Gas constant (R) = 8.341 mol^-1 K^-1
To calculate the rate constant (k) for a first-order reaction, we can use the Arrhenius equation:
k = A * exp(-Ea / (RT))
where exp is the exponential function.
Let's calculate the rate constant using the given values:
1. Calculate the value inside the exponential function:
Ea / (RT) = (98.6 kJ/mol) / (8.341 mol^-1 K^-1 * 303 K)
= 0.0418 mol / K
2. Calculate the exponential value:
exp(-Ea / (RT)) = exp(-0.0418)
≈ 0.959
3. Calculate the rate constant:
k = A * exp(-Ea / (RT))
= (4 x 10^13 collision/sec) * 0.959
= 3.83 x 10^13 collision/sec
However, the given options are in the order of 10^-3, so we need to convert the rate constant to the desired format:
k = 3.83 x 10^13 collision/sec
= 3.83 x 10^13 x 10^-6 x 10^3 collision/sec
= 3.83 x 10^-3 x 10^3 collision/sec
= 3.83 x 10^-3 x 10^3 x 10^3 mol^-1 sec^-1
= 3.83 x 10^3 x 10^3 x 10^-3 mol^-1 sec^-1
= 3.83 x 10^3 mol^-1 sec^-1
Comparing this value with the given options, we find that the correct answer is option 'c':
k = 3.83 x 10^3 mol^-1 sec^-1
≈ 4.07 x 10^-4 mol^-1 sec^-1
Therefore, the correct answer is option 'c', 4.07 x 10^-4.
Free Test
FREE
| Start Free Test |
Community Answer
For a certain reaction the values of Arrhenius factor and Activation e...
Given,
Arrhenius factor(A) = 4 x 1013 collisions/sec
Activation energy (Ea)=98.6KJ/mol=98.6 x 103J/mol, T=303 K
log K = log A – (Ea/2.303RT)
log K = log (4 x 1013) – (98.6 x 103)/(2.303 x 8.314 x 303)
log K = 13.6020 – (98.6 x 103/5801.584)
log k = -3.39
K = 10-3.39
K = 4.07 x 10-4.
Arrhenius factor(A) = 4 x 1013 collisions/sec
Activation energy (Ea)=98.6KJ/mol=98.6 x 103J/mol, T=303 K
log K = log A – (Ea/2.303RT)
log K = log (4 x 1013) – (98.6 x 103)/(2.303 x 8.314 x 303)
log K = 13.6020 – (98.6 x 103/5801.584)
log k = -3.39
K = 10-3.39
K = 4.07 x 10-4.
|
Explore Courses for Chemistry exam
|
|
Similar Chemistry Doubts
For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer?
Question Description
For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct 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 For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct 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 For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer?.
For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct 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 For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct 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 For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer?.
Solutions for For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
Download more important topics, notes, lectures and mock test series for Chemistry Exam by signing up for free.
Here you can find the meaning of For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer?, a detailed solution for For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice For a certain reaction the values of Arrhenius factor and Activation energy are 4 x 1013 collision/sec and 98.6KJ/mol at 303K. Calculate the rate constant if reaction is 1st order?( R=8.341mol-1K-1)a)6.07 x 10-3b)3.02 x 10-5c)4.07 x 10-4d)7.42 x 10-3Correct answer is option 'C'. Can you explain this answer? tests, examples and also practice Chemistry tests.
|
|
Explore Courses for Chemistry exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup