Under isothermal conditions, the volumes of ideal gas \(A\) and actual gas \(B\) grow from \(V\) to \(2V\). The increase in internal energy:

1.	will be the same in both \(A\) and \(B\).
2.	will be zero in both the gases.
3.	of \(B\) will be more than that of \(A\).
4.	of \(A\) will be more than that of \(B\).

The specific heat of a gas in an isothermal process is: 

The latent heat of vaporisation of water is 2240 J/gm. If the work done in the process of expansion of 1 g is 168 J, then increase in internal energy is 

(1) 2408 J

(2) 2240 J

(3) 2072 J

(4) 1904 J

A cylinder fitted with a piston contains 0.2 moles of air at temperature 27°C. The piston is pushed so slowly that the air within the cylinder remains in thermal equilibrium with the surroundings. Find the approximate work done by the system if the final volume is twice the initial volume 

(1) 543 J

(2) 345 J

(3) 453 J

(4) 600 J

If a cylinder containing a gas at high pressure explodes, the gas undergoes -

(1) Reversible adiabatic change and fall of temperature

(2) Reversible adiabatic change and rise of temperature

(3) Irreversible adiabatic change and fall of temperature

(4) Irreversible adiabatic change and rise of temperature

The work done in an adiabatic change in a gas depends only on

(1) Change is pressure

(2) Change is volume

(3) Change in temperature

(4) None of the above

In adiabatic expansion 

(1) ΔU = 0

(2) ΔU = negative

(3) ΔU = positive

(4) ΔW = zero

The pressure and density of a diatomic gas $(\gamma =7/5)$ changes adiabatically from (P, d) to (P', d'). If $\frac{d\text{'}}{d}=32$, then $\frac{P\text{'}}{P}$ should be: 

An ideal gas at 27°C is compressed adiabatically to $\frac{8}{27}$ of its original volume. If $\gamma =\frac{5}{3}$, then the rise in temperature is

(1) 450 K

(2) 375 K

(3) 225 K

(4) 405 K

Two identical samples of a gas are allowed to expand, (i) isothermally and (ii) adiabatically. The work done will be: