(a) 2 mole of an ideal monoatomic gas at 27°C expands reversibly and adiabatically from a volume of 20 dm to a volume of 40 dm. Calculate q. AU, W and AH. Given CR= 4/3
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- What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?A sample consisting of 1.00 mol Ar is expanded isothermally at 20 degrees celsius from 10 dm^3 to 30dm^3 (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, and (c) freely aka - against zero external pressure. For the three processes calculate q,w, and delta U
- One mole of a monatomic ideal gas goes through the cycle indicated in the figure according to stages 1,2 and 3 and involving states A, B and C. Assuming that all stages are reversible. CV = 3 / 2R. Calculate Q, W, ΔU and ΔH for each process and for the cycle.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.)An ideal monatomic gas expands adiabatically from 0.500 m3 to 1.57 m3. If the initial pressure and temperature are 1.30 ✕ 105 Pa and 350 K, respectively, find the number of moles in the gas, the final gas pressure (Pa), the final gas temperature (in K), and the work done on the gas (in J).
- A sample of carbon dioxide of mass 2.45 g at 27.0 °C is allowed to expand reversibly and adiabatically from 500 cm3 to 3.00 dm3. What is the work done by the gas?Calculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?A sample of 2.2 mol CO2(g) is originally confined in 15 dm3 at 280 K and then undergoes adiabatic expansion against a constant pressure of 78.5 kPa until the volume has increased by a factor of 4.0. Calculate ΔT. (The final pressure of the gas is not necessarily 78.5 kPa.)
- If 6.00 mol argon in a 100-L vessel initially at 300 K iscompressed adiabatically (q =0) and irreversibly until afinal temperature of 450 K is reached, calculate the energychange of the gas, the heat added to the gas, and the workdone on the gas.PHYSICALCHEMISTRY_SHOWSOLUTION:A sample consisting of 2.5 mol of perfect gas molecules with Cp,m = 29.4 J K –1 mol–1 is initially at 303 kPa and 335 K. It undergoes reversible adiabatic expansion until its pressure reaches 250 kPa. Calculate the final volume and temperature and the work done. ANSWER:[w = -9.00x102 J]A gas obeying the equation of state p(V − nb) = nRT is subjected to a Joule–Thomson expansion. Will the temperature increase, decrease, or remain the same?