Backn moles of a diatomic gas with Cv = 5/2 R has initial pressure pi and volume Vi. The gas undergoes a process in which the pressure is directly proportional to the volume until the rms speed of the molecules has doubled. How much heat does this process require? Give your answer in terms of n, pi and Vi.
0.10 mol of nitrogen gas follow the two processes shown in FIGURE P19.58. How much heat is required for each?
One cylinder in the diesel engine of a truck has an initial volume of 600 cm3. Air is admitted to the cylinder at 30°C and a pressure of 1.0 atm. The piston rod then does 400 J of work to rapidly compress the air. What are its final temperature and volume?
A gas cylinder holds 0.10 mol of O₂ at 150°C and a pressure of 3.0 atm. The gas expands adiabatically until the volume is doubled. What are the final pressure?
A gas cylinder holds 0.10 mol of O₂ at 150°C and a pressure of 3.0 atm. The gas expands adiabatically until the pressure is halved. What are the final temperature?
FIGURE P19.62 shows a thermodynamic process followed by 120 mg of helium. How much work is done on the gas during each of the three segments?
The volume of a gas is halved during an adiabatic compression that increases the pressure by a factor of 2.5. What is the specific heat ratio γ?
14 g of nitrogen gas at STP are adiabatically compressed to a pressure of 20 atm. What is the compression ratio Vmax/Vmin?
A monatomic gas is adiabatically compressed to 1/8 of its initial volume. Does each of the following quantities change? If so, does it increase or decrease, and by what factor? If not, why not? The thermal energy of the gas.
A monatomic gas is adiabatically compressed to 1/8 of its initial volume. Does each of the following quantities change? If so, does it increase or decrease, and by what factor? If not, why not? The molar specific heat at constant volume.
An experiment you're designing needs a gas with γ = 1.50. You recall from your physics class that no individual gas has this value, but it occurs to you that you could produce a gas with γ = 1.50 by mixing together a monatomic gas and a diatomic gas. What fraction of the molecules need to be monatomic?
A cylinder contains mol of helium at °C. If the gas is ideal, what is the change in its internal energy in part (a)? In part (b)? How do the two answers compare? Why?
(a) How much heat is needed to raise the temperature to °C while keeping the volume constant? Draw a -diagram for this process.
(b) If instead the pressure of the helium is kept constant, how much heat is needed to raise the temperature from °C to °C? Draw a -diagram for this process.
A cylinder contains mol of helium at °C. What accounts for the difference between your answers to parts (a) and (b)? In which case is more heat required? What becomes of the additional heat?
(a) How much heat is needed to raise the temperature to °C while keeping the volume constant? Draw a -diagram for this process.
(b) If instead the pressure of the helium is kept constant, how much heat is needed to raise the temperature from °C to °C? Draw a -diagram for this process.
A cylinder contains mol of helium at °C. How much heat is needed to raise the temperature to °C while keeping the volume constant? Draw a -diagram for this process.
(II) A 1.00-mol sample of an ideal diatomic gas, originally at 1.00 atm and 20°C, expands adiabatically to 1.75 times its initial volume. What are the final pressure and temperature for the gas? (Assume no molecular vibration.)