NEET Exam > NEET Questions > 5 mole of an ideal gas expand reversibly from...
Start Learning for Free
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K?
Most Upvoted Answer
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80d...
**Given Data:**
- Number of moles (n) = 5 mol
- Initial volume (V1) = 8 dm^3
- Final volume (V2) = 80 dm^3
- Temperature (T) = 300 K
**Calculating Change in Entropy:**
The change in entropy (ΔS) of an ideal gas during an isothermal and reversible expansion can be calculated using the equation:
ΔS = nR ln(V2/V1)
where:
- n is the number of moles of the gas
- R is the molar gas constant (8.314 J/(mol·K))
- ln is the natural logarithm function
- V2/V1 is the ratio of final volume to initial volume
**Substituting the given values:**
ΔS = 5 mol * 8.314 J/(mol·K) * ln(80 dm^3 / 8 dm^3)
**Calculating the ln(80/8):**
ln(80/8) = ln(10) = 2.3026
**Substituting back into the equation:**
ΔS = 5 mol * 8.314 J/(mol·K) * 2.3026
**Simplifying:**
ΔS = 95.73 J/K
Therefore, the change in entropy is 95.73 J/K.
**Answer:**
The correct option is C) 95.73 J/K.
- Number of moles (n) = 5 mol
- Initial volume (V1) = 8 dm^3
- Final volume (V2) = 80 dm^3
- Temperature (T) = 300 K
**Calculating Change in Entropy:**
The change in entropy (ΔS) of an ideal gas during an isothermal and reversible expansion can be calculated using the equation:
ΔS = nR ln(V2/V1)
where:
- n is the number of moles of the gas
- R is the molar gas constant (8.314 J/(mol·K))
- ln is the natural logarithm function
- V2/V1 is the ratio of final volume to initial volume
**Substituting the given values:**
ΔS = 5 mol * 8.314 J/(mol·K) * ln(80 dm^3 / 8 dm^3)
**Calculating the ln(80/8):**
ln(80/8) = ln(10) = 2.3026
**Substituting back into the equation:**
ΔS = 5 mol * 8.314 J/(mol·K) * 2.3026
**Simplifying:**
ΔS = 95.73 J/K
Therefore, the change in entropy is 95.73 J/K.
**Answer:**
The correct option is C) 95.73 J/K.
Community Answer
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80d...
Attention NEET Students!
To make sure you are not studying endlessly, EduRev has designed NEET study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in NEET.
|
Explore Courses for NEET exam
|
|
Similar NEET Doubts
Top Courses for NEETView all
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K?
Question Description
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K?.
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K?.
Solutions for 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? in English & in Hindi are available as part of our courses for NEET.
Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.
Here you can find the meaning of 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? defined & explained in the simplest way possible. Besides giving the explanation of
5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K?, a detailed solution for 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? has been provided alongside types of 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? theory, EduRev gives you an
ample number of questions to practice 5 mole of an ideal gas expand reversibly from a volume of 8dm^3 to 80dm^3 at a temperature of 300K. The change in entropy is A) 41.57J/K B) -95.73J/K C) 95.73J/K D) -41.57J/K? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET 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