BackA scuba diver releases a 3.60-cm-diameter (spherical) bubble of air from a depth of 14.0 m. Assume the temperature is constant at 298 K, and that the air behaves as an ideal gas. Apply the first law of thermodynamics to the bubble, and find the work done by the air in rising to the surface, the change in its internal energy, and the heat added or removed from the air in the bubble as it rises. Take the density of water to be 1000 kg/m3.
(I) An ideal gas expands isothermally, performing 4.30 x 103 J of work in the process. Calculate the heat absorbed during this expansion.
Two cylinders each contain 0.10 mol of a diatomic gas at 300 K and a pressure of 3.0 atm. Cylinder A expands isothermally and cylinder B expands adiabatically until the pressure of each is 1.0 atm. What are the final temperature and volume of each?
500 J of heat energy are transferred to a gas during a process in which the gas expands at constant pressure from 400 cm3 to 800 cm3. The gas's thermal energy increases by 300 J during this process. What is the gas pressure?
(II) How much work is done by a pump to slowly compress, isothermally, 3.20 L of nitrogen at 0°C and 1.00 atm to 1.80 L at 0°C?
A heat engine takes a diatomic gas around the cycle shown in Fig. 20–23. Calculate the heat input into the gas during the constant volume process from points b to c.
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 volume?
The volume of a gas is halved during an adiabatic compression that increases the pressure by a factor of 2.5. By what factor does the temperature increase?
(I) An ideal gas expands isothermally, performing 4.30 x 103 J of work in the process. Calculate the change in internal energy of the gas, and