Calculate the value of AS for three moles of an ideal gas compressed reversibly and isothermally from 75 Liters to 2.5 Liters.

Consider work, heat, and internal energy. Explain the molecular basis for each. Which are state and which are path functions? Provide reasoning to support your claims.

Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo

Suppose that one of water at its boiling point is kept in a cylinder that has frictionless piston. For equilibrium to be established, a pressure is maintained above the piston. If the piston sweeps out a volume of  0 dm3. Calculate  the work done by the system for the following paths: Free expansion Reversible expansion against constant pressure of 4.0 atm Isothermal reversible expansion with initial volume = 0.80 dm3.       When 2.0 mol of CO2 is heated at a constant pressure of 1.25 atm, its temperature increases from 280.00 K to 307.00 K. The heat (q) absorbed during this process is determined to be 2.0 kJ. Calculate (a) ΔH for this process (b) The molar heat capacity of CO2 at constant pressure (CP,m)       (Hint: you can assume that CP,m is constant over this temperature range and that the CO2behaves ideally).             (c) ΔU.       Heat capacity of a material is temperature dependent. The T-dependence of the molar heat capacities of water (H2O(l)), H2(g) and O2(g) can be…

Consider the free, isothermal (constant T) expansion of an ideal gas. "Free" means that the external force is zero, perhaps because a stopcock has been opened and the gas is allowed to expand into a vacuum. Calculate AU for this irreversible process. Show that q sion is also adiabatic (q = 0) for an ideal gas. This is analogous to a classic experiment first performed by Joule. 0, so that the expan-

Silver, Water and Aluminum

Please don't provide handwritten solution ......

Part A: 10 moles of ideal gas initially at 10 atm and 250 K is expanded isothermally and reversibly to a final pressure of 2 atm. Calculate W; U; and Q in Joules. Part B: The same gas in part A, starting in the same initial state, is expanded isothermally against a constant external pressure of 2 atm, to a final pressure of 2 atm. Calculate W; U; and Q in Joules for this irreversible process. Part C: The same gas in part B, starting in the same initial state, is expanded isothermally to a nal pressure of 2 atm. The process is carried out in 4 stages. First the gas is expanded against a constant pressure of 8 atm, to 8 atm. Then the gas is expanded against a constant pressure of 6 atm, to 6 atm. Then the gas is expanded against a constant pressure of 4 atm, to 4 atm. Finally, the gas is expanded against a constant pressure of 2 þtm, to 2 atm. Calculate W; U; and Q in Joules for the 4-step process.