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Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1 and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas is
- a)332 J
- b)80.3 J
- c)303 J
- d)880 J
Correct answer is 'D'. Can you explain this answer?
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Verified Answer
Four moles of an ideal diatomic gas is heated at constant volume from ...
The value of Cp is 30.3
and as Cp-Cv = R(8.3)
hence Cv = 30.3-8.3
Cv is 22
change in internal energy = no of moles × Cv × change in temperature
hence
change in internal energy = 22 × 4 × 10
= 880j
Hence Option D is correct.
and as Cp-Cv = R(8.3)
hence Cv = 30.3-8.3
Cv is 22
change in internal energy = no of moles × Cv × change in temperature
hence
change in internal energy = 22 × 4 × 10
= 880j
Hence Option D is correct.
Most Upvoted Answer
Four moles of an ideal diatomic gas is heated at constant volume from ...
The value of Cp is 30.3
and as Cp-Cv = R(8.3)
hence Cv = 30.3-8.3
Cv is 22
change in internal energy = no of moles × Cv × change in temperature
hence
change in internal energy = 22 × 4 × 10
= 880
and as Cp-Cv = R(8.3)
hence Cv = 30.3-8.3
Cv is 22
change in internal energy = no of moles × Cv × change in temperature
hence
change in internal energy = 22 × 4 × 10
= 880
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Community Answer
Four moles of an ideal diatomic gas is heated at constant volume from ...
°C to 60°C. The specific heat capacity of diatomic gas at constant volume is 20.8 J/mol.K.
To calculate the change in internal energy of the gas, we can use the formula:
ΔU = nCvΔT
Where ΔU is the change in internal energy, n is the number of moles of the gas, Cv is the specific heat capacity at constant volume, and ΔT is the change in temperature.
ΔU = 4 mol x 20.8 J/mol.K x (60°C - 20°C)
ΔU = 4 mol x 20.8 J/mol.K x 40°C
ΔU = 3328 J
Therefore, the change in internal energy of the gas is 3328 J.
To calculate the change in internal energy of the gas, we can use the formula:
ΔU = nCvΔT
Where ΔU is the change in internal energy, n is the number of moles of the gas, Cv is the specific heat capacity at constant volume, and ΔT is the change in temperature.
ΔU = 4 mol x 20.8 J/mol.K x (60°C - 20°C)
ΔU = 4 mol x 20.8 J/mol.K x 40°C
ΔU = 3328 J
Therefore, the change in internal energy of the gas is 3328 J.
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Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer?
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Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer?.
Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer?.
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Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer?, a detailed solution for Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? has been provided alongside types of Four moles of an ideal diatomic gas is heated at constant volume from 20° C to 30° C. The molar specific heat of the gas at constant pressure (Cp) is 30.3 Jmol-1K-1and the universal gas constant (R) is 8.3 Jmol-1K-1. The increase in internal energy of the gas isa)332 Jb)80.3 Jc)303 Jd)880 JCorrect answer is 'D'. Can you explain this answer? theory, EduRev gives you an
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