Two cylinders of equal size are filled with equal amount of ideal diatomic gas at room temperature. Both the cylinders are fitted with pistons. In cylinder A the piston is free to move, while in cylinder B the piston is fixed. When the same amount of heat is added to cylinder A, it raises by 20 K. What will be the rise temperature of gas in cylinder B?
Correct answer: A. 28 K
- A. 28 K
- B. 20 K
- C. 15 K
- D. 10 K
Explanation
Option A is correct.Given data: For diatomic Cp/Cv=7/5Find out:∆T2 =?We know that For gas in cylinder A, Q=nCp∆T1For gas in cylinder B, Q=nCp∆T2∆T2=Cp/Cv∆T=7/5x20=28K
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About Molar Specific Heat of a Gas
Molar specific heat is the heat required to raise the temperature of one mole of a gas by one kelvin, expressed through Q = nCΔT. Questions compare the constant volume value Cv with the constant pressure value Cp, apply the ideal gas relation Cp − Cv = R, and identify how the thermodynamic process affects heat capacity.
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