1. Air at 20 °C is allowed to expand under adiabatic conditions until its pressure has fallen to one-third of its original value.
What is the final temperature of the air? (Ratio of the principal specific heats of air = 1.4)
2. A certain volume of helium at 15°C is expanded adiabatically until its volume is trebled.
Calculate the temperature of the gas immediately after the expansion has taken place. (Ratio of the principal specific heat capacities of helium = 1.67)
3. Some nitrogen at 20°C is expanded isothermally to twice its original volume. It is then cooled at constant volume to -10°C and finally compressed adiabatically to its original pressure and volume.
(a) Draw a pV diagram to show this change.
(b) Calculate the pressure after the isothermal expansion.
(c) Calculate the pressure after the cooling at constant volume.
4. The density of neon at 27°C and a pressure of 1.00x105 Pa is 0.90 kgm-3. Calculate the mass of neon in a neon discharge tube of volume 250 cm3 if the pressure inside it is 1.00x105 Pa at a temperature of 150 °C
5. Two identical glass bulbs are joined with a thin glass tube and filled with air which is initially at 20°C. What will the pressure in the apparatus become if one bulb is immersed in steam and the other in melting ice?
6. When a gas expands adiabatically it does work on its surroundings although there is no heat input to the gas. Where does this energy come from?
7. A mass of 1 g of hydrogen at 20°C and 105 Pa has its volume halved by an adiabatic change. Calculate the change in the internal energy of the gas. (Ideal gas constant = 8.31 J mol-1; ratio of .the principal specific heats for hydrogen = 1.40)
8. A mass of air with an initial volume of 5 litres at a temperature of 0°C and a pressure of 105 Pa is compressed isothermally to 2.5 litres, and then allowed to expand adiabatically to 12.5 litres.
Show the process on a PV diagram and calculate the final pressure and temperature of the air. At what volume was the pressure momentarily atmospheric? (Assume γ for air = 1.40.)
9. State the first law of thermodynamics. How is the equation modified for:
(a) an adiabatic change
(b) an input of heat at constant volume. Explain how the composition of the term for internal energy for a real gas differs from that for an ideal one.