If an ideal gas undergoes two processes at constant volumes as shown in the pressure-temperature (P-T) diagram, then:
1. =
2. >
3. <
4.
The internal energy of an ideal gas increases in:
1. Adiabatic expansion
2. Adiabatic compression
3. Isothermal expansion
4. Isothermal compression
0.04 mole of an ideal monatomic gas is allowed to expand adiabatically so that its temperature changes from 800 K to 500 K. The work done during expansion is nearly equal to:
1. | \(129.6\) J | 2. | \(-129.6\) J |
3. | \(149.6\) J | 4. | \(-149.6\) J |
Which of the following is true for the molar heat capacity of an ideal gas?
1. | It cannot be negative. |
2. | It has only two values \(\left(C_P \text { and } C_V\right)\). |
3. | It can have any value. |
4. | It cannot be zero. |
A heat engine is working between 200 K and 400 K. The efficiency of the heat engine may be:
1. 20%
2. 40%
3. 50%
4. All of these
The work done by an ideal diatomic gas in its sudden expansion is 20 J. The change in the internal energy of the gas will be:
1. 20 J
2. 0 J
3. J
4. J
In the cyclic process shown in the pressure-volume \((P-V)\) diagram, the change in internal energy is equal to:
1.
2.
3.
4. zero
Heat is supplied to a diatomic gas in an isochoric process. The ratio is: (symbols have usual meanings)
1. 5 : 3
2. 5: 2
3. 1: 1
4. 5: 7
When a system is moved from state a to state b along the path acb, it is discovered that the system absorbs 200 J of heat and performs 80 J of work. Along the path adb, heat absorbed Q = 144 J. The work done along the path adb is:
1. | 6 J | 2. | 12 J |
3. | 18 J | 4. | 24 J |
The variation of molar heat capacity at constant volume with temperature T for a monatomic gas is:
1. | 2. | ||
3. | 4. |