HC Verma - Concepts of Physics Part 2

Book: HC Verma - Concepts of Physics Part 2

Chapter: 27. Specific Heat Capacities of Gases

Subject: Physics - Class 12th

Q. No. 3 of Objective I

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The value of CP – CV is 1.00 R for a gas sample in state A and is 1.08R in state B. Let PA, PB denote the pressures and TA, and TB denote the temperatures of the states A and B respectively. Most likely

For gas in state A, Cp - Cv = R. This represents an ideal gas. Now, for an ideal gas, we require very high temperature and very low pressure compared to a real gas


For gas in state B, Cp - Cv = 1.08R, which represents a real gas. Since gas A was ideal, its pressure must be much lower than that of B and temperature must be much higher than that of A.


Hence, we require the condition pA < pB and TA > TB. This is given by option (a).


Options (b), (c) and (d) are incorrect because none of those satisfies the conditions for an ideal gas.

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Chapter Exercises

Short Answer
Objective I
Objective II
Exercises

More Exercise Questions

1

Work done by a sample of an ideal gas in a process A is double the work done in another process B. The temperature rises through the same amount in the two processes. If CA and CB be the molar heat capacities for the two processes.
2

For a solid with a small expansion coefficient,
3

The value of CP – CV is 1.00 R for a gas sample in state A and is 1.08R in state B. Let PA, PB denote the pressures and TA, and TB denote the temperatures of the states A and B respectively. Most likely
4

Let CV and CP denote the molar heat capacities of an ideal gas at constant volume and constant pressure respectively. Which of the following is a universal constant?
5

70 calories of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30°C to 35°C. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is
6

The molar heat capacity for the process shown in the figure is
7

The molar heat capacity for the process shown in the figure is
8

In an isothermal process on an ideal gas, the pressure increases by 0.5%. The volume decreases by about
9

In an adiabatic process on gas with γ = 1.4, the pressure is increased by 0.5%. The volume decreases by about
10

Two samples A and B are initially kept in the same state. Sample A is expanded through an adiabatic process and sample B through an isothermal process. The final volumes of the samples are the same. The final pressures in A and B are pA and PB respectively.
11

Let Ta and Tb be the final temperatures of the samples A and B respectively in the previous question.
12

Let ΔWa and ΔWb be the work done by the systems A and B respectively in the previous question.
13

The molar heat capacity of oxygen gas at STP is nearly 2.5R. As the temperature is increased, it gradually increases and approaches 3.5R. The most appropriate reason for this behaviour is that at high temperatures.