NEET Exam > NEET Questions > Two moles of an ideal gas are compressed at 3...
Start Learning for Free
Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy is
- a)1.46 KJ-mol⁻1
- b)3.46 KJ-mol⁻1
- c)5.46 KJ-mol⁻1
- d)7.46 KJ-mol⁻1
Correct answer is 'B'. Can you explain this answer?
Most Upvoted Answer
Two moles of an ideal gas are compressed at 300 K from a pressure of 1...
Change in Free Energy Formula:
The change in free energy (∆G) of a system can be calculated using the equation:
∆G = ∆H - T∆S
Where:
∆G = Change in Free Energy
∆H = Change in Enthalpy
T = Temperature in Kelvin
∆S = Change in Entropy
Given Information:
Number of moles of gas (n) = 2
Initial pressure (Pi) = 1 atm
Final pressure (Pf) = 2 atm
Initial temperature (Ti) = 300 K
Step 1: Calculate the Change in Enthalpy (∆H)
Since the gas is an ideal gas, we can use the ideal gas equation to determine the change in enthalpy:
∆H = nR∆T
Where:
R = Gas constant (8.314 J/mol·K)
∆T = Change in temperature (Tf - Ti)
Since the temperature is constant in this case, ∆T = 0. Therefore, the change in enthalpy (∆H) is equal to zero.
Step 2: Calculate the Change in Entropy (∆S)
The change in entropy can be calculated using the equation:
∆S = nRln(Pf/Pi)
Where:
ln = Natural logarithm
Plugging in the values:
∆S = (2 moles)(8.314 J/mol·K)ln(2 atm/1 atm)
∆S = 2(8.314 J/mol·K)ln(2)
∆S ≈ 2(8.314 J/mol·K)(0.6931)
∆S ≈ 11.57 J/mol·K
Step 3: Calculate the Change in Free Energy (∆G)
Using the equation:
∆G = ∆H - T∆S
Plugging in the values:
∆G = 0 - (300 K)(11.57 J/mol·K)
∆G = -3471 J/mol
Converting to kilojoules:
∆G ≈ -3.47 kJ/mol
Answer:
The change in free energy (∆G) is approximately -3.47 kJ/mol.
The change in free energy (∆G) of a system can be calculated using the equation:
∆G = ∆H - T∆S
Where:
∆G = Change in Free Energy
∆H = Change in Enthalpy
T = Temperature in Kelvin
∆S = Change in Entropy
Given Information:
Number of moles of gas (n) = 2
Initial pressure (Pi) = 1 atm
Final pressure (Pf) = 2 atm
Initial temperature (Ti) = 300 K
Step 1: Calculate the Change in Enthalpy (∆H)
Since the gas is an ideal gas, we can use the ideal gas equation to determine the change in enthalpy:
∆H = nR∆T
Where:
R = Gas constant (8.314 J/mol·K)
∆T = Change in temperature (Tf - Ti)
Since the temperature is constant in this case, ∆T = 0. Therefore, the change in enthalpy (∆H) is equal to zero.
Step 2: Calculate the Change in Entropy (∆S)
The change in entropy can be calculated using the equation:
∆S = nRln(Pf/Pi)
Where:
ln = Natural logarithm
Plugging in the values:
∆S = (2 moles)(8.314 J/mol·K)ln(2 atm/1 atm)
∆S = 2(8.314 J/mol·K)ln(2)
∆S ≈ 2(8.314 J/mol·K)(0.6931)
∆S ≈ 11.57 J/mol·K
Step 3: Calculate the Change in Free Energy (∆G)
Using the equation:
∆G = ∆H - T∆S
Plugging in the values:
∆G = 0 - (300 K)(11.57 J/mol·K)
∆G = -3471 J/mol
Converting to kilojoules:
∆G ≈ -3.47 kJ/mol
Answer:
The change in free energy (∆G) is approximately -3.47 kJ/mol.
Free Test
FREE
| Start Free Test |
Community Answer
Two moles of an ideal gas are compressed at 300 K from a pressure of 1...
Free energy change =2.303×2×8.314×300log(2/1)
|
Explore Courses for NEET exam
|
|
Top Courses for NEETView all
Question Description
Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer?.
Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer?.
Solutions for Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? 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 Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer?, a detailed solution for Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? has been provided alongside types of Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice Two moles of an ideal gas are compressed at 300 K from a pressure of 1 atm to a pressure of 2 atm. The change in free energy isa)1.46 KJ-mol⁻1b)3.46 KJ-mol⁻1c)5.46 KJ-mol⁻1d)7.46 KJ-mol⁻1Correct answer is 'B'. Can you explain this answer? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup to see your scores
go up
within 7 days!
within 7 days!
Takes less than 10 seconds to signup