\(ABCA\) is a cyclic process. Its \(P\text-V\) graph would be:
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If the ratio of specific heat of a gas at constant pressure to that at constant volume is , the change in internal energy of a mass of gas, when the volume changes from V to 2V at constant pressure, P is:
1. | 2. | PV | |
3. | 4. |
The degree of freedom per molecule for a gas on average is 8. If the gas performs 100 J of work when it expands under constant pressure, then the amount of heat absorbed by the gas is:
1. 500 J
2. 600 J
3. 20 J
4. 400 J
The pressure in a monoatomic gas increases linearly from 4 atm to 8 atm when its volume increases from 0.2 m to 0.5 m. The increase in internal energy will be:
1. | 480 kJ | 2. | 550 kJ |
3. | 200 kJ | 4. | 100 kJ |
If in the thermodynamic process shown in the figure, the work done by the system along A B C is 50 J and the change in internal energy during C A is 30 J, then the heat supplied during A B C is:
1. | 50 J | 2. | 20 J |
3. | 10 J | 4. | 80 J |
In the \((P\text-V)\) diagram shown, the gas does \(5~\text J\) of work in the isothermal process \(ab\) and \(4~\text J\) in the adiabatic process \(bc.\) What will be the change in internal energy of the gas in the straight path from \(c\) to \(a?\)
1. \(9~\text J\)
2. \(1~\text J\)
3. \(4~\text J\)
4. \(5~\text J\)
A horizontal cylinder has two sections of unequal cross-sections in which two pistons, A and B, can move freely. The pistons are joined by a string. Some gas is trapped between the pistons. If this gas is heated, the pistons will:
1. | move to the left. |
2. | move to the right. |
3. | remain stationary. |
4. | move either to the left or to the right depending on the initial pressure of the gas. |
The pressure of a monoatomic gas increases linearly from \(4\times 10^5~\text{N/m}^2\) to \(8\times 10^5~\text{N/m}^2\) when its volume increases from \(0.2 ~\text m^3\) to \(0.5 ~\text m^3.\) The work done by the gas is:
1. \(2 . 8 \times10^{5}~\text J\)
2. \(1 . 8 \times10^{6}~\text J\)
3. \(1 . 8 \times10^{5}~\text J\)
4. \(1 . 8 \times10^{2}~\text J\)
An ideal gas is taken through the cycle \(A\rightarrow B\rightarrow C\rightarrow A\) as shown in the figure below. If the net heat supplied to the gas is \(10~\text{J}\), then the work done by the gas in the process \(B\rightarrow C\) is:
1. | \(-10~\text{J}\) | 2. | \(-30~\text{J}\) |
3. | \(-15~\text{J}\) | 4. | \(-20~\text{J}\) |
One mole of an ideal gas expands at a constant temperature of \(300~\text{K}\) from an initial volume of \(10\) litres to a final volume of \(20\) litres.
The work done in expanding the gas is equal to:
(\(R = 8.31\) J/mole-K)
1. \(750~\text{J}\)
2. \(1728~\text{J}\)
3. \(1500~\text{J}\)
4. \(3456~\text{J}\)