# The molar specific heats of an ideal gas at constant pressure and volume are denoted by $$C_P$$ and $$C_V,$$ respectively. If $$\gamma =\frac{C_P}{C_V}$$ and $$R$$ is the universal gas constant, then $$C_V$$ is equal to: 1. $$\frac{R}{\gamma -1}$$ 2. $$\frac{\gamma -1}{R}$$ 3. $$\gamma R$$ 4. $$\frac{\left ( \gamma -1 \right )R}{\left ( \gamma +1 \right )}$$

Subtopic:  Molar Specific Heat |
88%
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AIPMT - 2013
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During an adiabatic process, the pressure of a gas is found to be proportional to the cube of its temperature. The ratio of $$\frac{C_P}{C_V}$$ for the gas is:
1. $$2$$
2. $$5/3$$
3. $$3/2$$
4. $$4/3$$
Subtopic:  Types of Processes |
71%
From NCERT
AIPMT - 2013
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A thermodynamic system is taken through the cycle $$\mathrm{ABCD}$$ as shown in the figure. Heat rejected by the gas during the cycle is:

1. $$2 {PV}$$
2. $$4{PV}$$
3. $$\frac{1}{2}{PV}$$
4. $$PV$$

Subtopic:  Cyclic Process |
74%
From NCERT
AIPMT - 2012
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One mole of an ideal gas goes from an initial state $$A$$ to the final state $$B$$ with two processes. It first undergoes isothermal expansion from volume $$V$$ to $$3V$$ and then its volume is reduced from $$3V$$ to $$V$$ at constant pressure. The correct $$(P-V)$$ diagram representing the two processes is:

 1 2 3 4

Subtopic:  Types of Processes |
81%
From NCERT
AIPMT - 2012
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When $$1$$ kg of ice at $$0^{\circ}$$ C melts into the water at $$0^{\circ}$$ C, the resulting change in its entropy, taking the latent heat of ice to be $$80$$ cal/gm, is:
1. $$8\times 10^4$$ cal/K
2. $$80$$ cal/K
3. $$293$$ cal/K
4. $$273$$ cal/K

Subtopic:  Second Law of Thermodynamics |
57%
From NCERT
AIPMT - 2011
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During an isothermal expansion, a confined ideal gas does -150 J of work against its surrounding. This implies that:

 1 300 J of heat has been added to the gas. 2 no heat is transferred because the process is isothermal. 3 150 J of heat has been added to the gas. 4 150 J of heat has been removed from the gas.

Subtopic:  First Law of Thermodynamics |
66%
From NCERT
AIPMT - 2011
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If $$\Delta U$$ and $$\Delta W$$ represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true?

 1 $$\Delta U=-\Delta W$$, in an adiabatic process 2 $$\Delta U=\Delta W$$ , in an isothermal process 3 $$\Delta U=\Delta W$$,  in an adiabatic process 4 $$\Delta U=-\Delta W$$, in an isothermal process
Subtopic:  First Law of Thermodynamics |
81%
From NCERT
AIPMT - 2010
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The internal energy change in a system that has absorbed $$2$$ kcal of heat and done $$500$$ J of work is:
1. $$8900$$ J
2. $$6400$$ J
3. $$5400$$ J
4. $$7900$$ J

Subtopic:  First Law of Thermodynamics |
78%
From NCERT
AIPMT - 2009
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In thermodynamic processes which of the following statements is not true?

 1 In an adiabatic process, the system is insulated from the surroundings. 2 In an isochoric process, pressure remains constant. 3 In an isothermal process, the temperature remains constant. 4 In an adiabatic process $$PV^\gamma=\mathrm{constant}.$$

Subtopic:  Types of Processes |
91%
From NCERT
AIPMT - 2009
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If $$Q$$, $$E$$, and $$W$$ denote respectively the heat added, the change in internal energy, and the work done in a closed cycle process, then:

 1 $$W=0$$ 2 $$Q=W=0$$ 3 $$E=0$$ 4 $$Q=0$$
Subtopic:  Cyclic Process |
77%
From NCERT
AIPMT - 2008
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