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:

Which is the correct statement ?

(1) For an isothermal change PV = constant

(2) In an isothermal process the change in internal energy must be equal to the work done

(3) For an adiabatic change $\frac{P_2}{P_1}={\left(\frac{{\displaystyle V_2}}{{\displaystyle V_1}}\right)}^{\gamma }$, where γ is the ratio of specific heats

(4) In an adiabatic process work done must be equal to the heat entering the system