2.50 moles of an ideal triatomic gas is expanded reversibly and isothermally ( 25 degrees Celsius ) from Pi = 5.00 atm to Pf = 1.00 atm. Sketch a diagram using a piston. Estimate the values of Vi , Vf, delta U, w, q, delta A, delta S, delta H and delta G.



2.50 moles of an ideal triatomic gas is expanded reversibly and isothermally ( 25 degrees Celsius...
Five moles of an ideal gas are expanded reversibly from a pressure of 5.0 atm to a pressure of 1.0 atm at a constant temperature of 298 K. ANSWER FOR Q= 19937.5J Calculate the value of delta S for the system??????? Calculate the value of delta S for the system?????????? Calculate the value of delta S total?????
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...
7.1.00 mol of an ideal gas at 27°C is expanded isothermally from an initial pressure of 3.00 atm to a final pressure of 1.00 atm in two ways: (a) reversibly; (b) against a constant external pressure of 1.00 atm Determine the values of ASsys, ASsur, AStot. Hint, you may need to begin by computing other functions such as q, w, AH etc. The temperature of the surroundings equals the temperature of the system.
1. a) One mole of an ideal gas at 298.15 K is expanded reversibly and isothermally from 1.0 L to 15 L. Determine the amount of work in Joules. b) Determine the work done in Joules when one mole of ideal gas is expanded irreversibly from 1.0 L to 15.0 L against a constant external pressure of 1.0 atm.
Five moles of nitrogen gas is expanded in a piston-cylinder assembly from an initial state of 3 bar and 88 ºC to a final pressure of 1 bar. You can assume nitrogen to behave as an ideal gas with a constant heat capacity CP =7R/2. a) If the expansion is carried out isothermally and reversibly, calculate Q, W, ΔH and ΔU. Draw the process on a pV diagram. Label the axis and the path clearly. b) If the expansion is...
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?
A piston containing 0.75 moles of a perfect gas at 25 degrees C
is moved isothermally from a starting volume of 8.305 L.
Calculate the work in joules if the piston is moved irreversibly
against a constant external pressure of 4.100 atm. We weren't
giving final volume so I am unsure of what to do. I tried to use
P1V1 = P2V2 because the final pressure is equal to external
pressure in an irreversible process. But then my final volume...
One mole of an ideal gas, with CV,m=1.5R, is expanded isothermally at 341 K from 8.00 bar to 3.20 bar against a constant external pressure equal to the final pressure. Calculate q, w, ΔU and ΔH. Assume the temperature of the surroundings is also 341 K. find q, u, Delta H, Delta U
A quantity of 6.0 moles of an ideal gas is reversibly heated atconstant volume from 17 degrees Celsius to 35 degrees Celsius.Calculate the entropy change. What would be the value of delta S if the heating were carried out irreversibly?
Two moles of an ideal gas occupy a volume V. The gas expands isothermally and reversibly to a volume 6 V. A)Is the velocity distribution changed by the isothermal expansion? B)Explain why ? C)Use the equation ΔS=klnw2/w1 to calculate the change in entropy of the gas. D)Use the equation ΔS=Q/T to calculate the change in entropy of the gas. Compare the result in part (d) to that obtained in part (c).