Problem 2
One mole of a monatomic ideal gas, initially at absolute temperature , is heated to in a constant-pressure process. Let be the gas constant; assume thermodynamic equilibrium throughout and no phase change. Define as work done by the gas and as heat absorbed, so the first law is . (a) Use the equation of state to find the volume change and work. (b) Calculate the internal-energy change from the molecular degrees of freedom. (c) Determine the heat transfer, check its sign, and explain how it is divided between raising internal energy and doing work.
problems.proof.stepOf
problems.proof.analysis
The gas expands while heating, so work, internal-energy change, and absorbed heat are all positive. Pressure remains constant and the gas follows the ideal-gas model.