An ideal gas follows a process described by the equation \(PV^2=\text{C}\) from the initial \((P_1, V_1, T_1)\) to final \((P_2, V_2, T_2)\) thermodynamics states, where \(\text{C}\) is a constant. Then:

1.	\(\text{If}~P_1>P_2~\text{then}~T_1<T_2\)
2.	\(\text{If}~V_2>V_1~\text{then}~T_2>T_1\)
3.	\(\text{If}~V_2>V_1~\text{then}~T_2<T_1\)
4.	\(\text{If}~P_1>P_2~\text{then}~V_1>V_2\)

A gas undergoes an isothermal process. The specific heat capacity of the gas in the process is:
1. infinity
2. \(0.5\)
3. zero
4. \(1\)

One mole of an ideal gas at an initial temperature of \(T\) K does \(6R\) joules of work adiabatically. If the ratio of specific heats of this gas at constant pressure and at constant volume is \(5/3\), the final temperature of the gas will be:
1. \((T-2.4)\) K
2. \((T+4)\) K
3. \((T-4)\) K
4. \((T+2.4)\) K

The initial pressure and volume of a gas are P and V respectively. First, its volume is expanded to 4V by an isothermal process and then compressed adiabatically to volume V. The final pressure will be (γ = 1.5):
1.  8P
2.  4P
3.  P
4.  2P

We consider a thermodynamic system. If ∆U represents the increase in its internal energy and W the work done by the system, which of the following statements is true?

If a gas changes volume from 2 litres to 10 litres at a constant temperature of 300K, then the change in its internal energy will be:

When volume changes from \(V\) to \(2V\) at constant pressure(\(P\)), the change in internal energy will be:
1. \(PV\)
2. \(3PV\)
3. \(\frac{PV}{\gamma -1}\)
4. \(\frac{RV}{\gamma -1}\)

An ideal gas heat engine operates in a Carnot cycle between 227ºC and 127ºC. It absorbs 6 × 10⁴ cals of heat at higher temperatures. The amount of heat converted to work will be?
1. 4.8 × 10⁴ cals
2. 2.4 × 10⁴ cals
3. 1.2 × 10⁴ cals
4. 6 × 10⁴ cals