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- 1) A sample containing 1.50 mol of an ideal gas with CV,m = 20.8 J K−1 mol−1isinitially at 230 kPa and 315 K. It undergoes a reversible adiabatic expansion until itspressure reaches 170 kPa. Calculate the final volume V2; the final temperature T2, andthe work w done by the system.A sample of nitrogen of mass 3.12 g at 23.0 °C is allowed to expand reversibly and adiabatically from 400 cm3 to 2.00 dm3. What is the work done by the gas?Two moles of a perfect gas with CV,m = 27.6 J K-1 mol-1 at 220 K and 200 kPa is compressed reversibly and adiabatically until the temperature reaches 255 K. Calculate q, w, ΔU, ΔH and the final pressure and volume.
- calculate the final temperature of a sample of carbon dioxide of mass 16.0g that is expanded reversibly and adiabatically from 500cm3 at 298.15K to 2dm3 if Cp,m is equal 37.11J/K.mol.Calculate the work done for the adiabatic compression of ethane from 150kPa to 600kPa at 20C. Assume ethane to be an ideal gas.Express the work of an isothermal reversible expansion of a van der Waals gas in reduced variables (Topic 1C) and find a definition of reduced work that makes the overall expression independent of the identity of the gas. Calculate the work of isothermal reversible expansion along the critical isotherm from Vc to xVc.
- Calculate the final pressure of a sample of water vapour that expands reversibly and adiabatically from 87.3 Torr and 500 cm3 to a final volume of 3.0 dm3. Take (gamma) γ = 1.3. ANs in t0rrOne mole of a perfect monatomic gas, initially at 300 K and a pressure 15.0 atm, expands to afinal pressure of 1.00 atm. Consider the expansion via each of the following paths: (a)isothermal and reversible, (b) isothermal and irreversible, (c) adiabatic and reversible, (d)adiabatic and irreversible. In these irreversible processes, the expansion occurs against anexternal pressure of 1.00 atm. For each case, calculate the values of q, w, ΔU and ΔH.One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)
- For H2(g), Cp,m is nearly constant at 20.4 J/mol K for temperatures in the range of 100 K to 400 K and low or moderate temperatures. Calculate q, w, and ∆U for the reversible adiabatic expansion of 12.0 g of H2 (g) from 1200 torr and 600 cm3 to a final volume of 800 cm3. After you solve the problem, state whether T of the H2 would increase or decrease during the process, and state your reasoning.Consider an equation of state for a gas given by: ?=1+(?/?? + ?/?2?) where B and C are constants and Z is the compressibility (compression) factor. Derive an expression for the work done in a reversible isothermal expansion from V1 to V2 at temperature T for one mole of the gas.5.00 mol of a perfect gas expand isothermally at 298 K from 2.00 dm3 to 12.00 dm3 Calculate the work done for an expansion against an external pressure of 200000 Pa: