
PChem 6. 2.00 mol of a perfect gas at 35°C is expanded reversibly and adiabatically to...
A sample of n moles of a monatomic ideal gas is expanded isothermally and reversibly at a constant temperature T from a volume V to 3V. Note that since the temperature of the gas is constant, the internal energy will remain constant. a) Write an expression for the change in entropy ΔS for the system. b) The sample has 7 moles of gas and is kept at a temperature of 305 K. The volume is changed from 0.065 m3 to...
1.3 mole of an ideal gas at 300 K is expanded isothermally and reversibly from a volume V to volume 4V. What is the change in entropy of the gas, in J/K?
3. A sample of 3.0 mole of a perfect gas at 25 °C expands from 5.0 L to 15.0 L. How much are the entropy changes of the system and the surroundings, and the total change in entropy in the following processes: (a) the gas expands reversibly and isothermally; (b)the gas expands isothermally but irreversibly against an external pressure of zero (Pex= 0), and (c) the gas expands adiabatically and reversibly. (20 pts)
4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and 25°C. Calculate the maximum work (in joules) that can be obtained when the gas is allowed to expand reversibly to a pressure of 1 bar; (a) (10pts) isothermally (b) (15pts) adiabatically The molar heat apacity of nitrogen at constant volume is 20.8 J/K mol. Assume that nitrogen behaves as an ideal gas
4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and...
A piston reversibly and adiabatically contracts 3.88 moles of ideal gas to one-tenth of its original volume, then expands back to the original conditions. It does this a total of five times. If the initial and final temperature of the gas is 27.5 degree C, calculate (a) the total work and (b) the total change in internal energy for the overall process.
A 12 m3 volume of ideal gas is expanded adiabatically. If the work done by the gas is 900 J what is the change in internal energy of the gas? The answer is -900J but I don't know how to get this answer.. Show all work! Thanks!
A sample of 1.00 mol of N2 gas is expanded adiabatically from a volume of 10.00 dm3 and a temperature of 400 K to a volume of 20.00 - 3 -dm3. Assume that nitrogen is ideal, with Cv,m = 5R/2. (i) Find the final temperature if the expansion is carried out reversibly. (ii) Calculate the final temperature if the expansion is carried out with a constant external pressure of 1.00 atm. (iii) Find the final temperature if the gas expands...
A 2.00 mol sample of an ideal gas with a molar specific heat of CV = 5 2 R always starts at pressure 1.50 ✕ 105 Pa and temperature 250 K. For each of the following processes, determine the final pressure (Pf, in kPa), the final volume (Vf, in L), the final temperature (Tf, in K), the change in internal energy of the gas (ΔEint, in J), the energy added to the gas by heat (Q, in J), and the...
The temperature of 2.00 mol of an ideal monatomic gas is raised 15.0 K at constant volume. What are (a) the work W done by the gas, (b) the energy transferred as heat Q , (c) the change ?Eint in the internal energy of the gas, and (d) the change ?K in the average kinetic energy per atom?
Properties of energy
1 mol of an ideal gas at initial conditions p,-150 kPa, Vi-20 L was compressed to p2 450 kPa through adiabatic reversible compression. Determine the work, heat, change of internal energy, enthalpy and entropy for the process. The gas heat capacity is Cpm-29.10 J K mol