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).
Two moles of an ideal gas occupy a volume V. The gas expands isothermally and reversibly...
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...
A 2.5 mole sample of an ideal gas expands reversibly and isothermally at 360 K until its volume is doubled. What is the increase in entropy of the gas?
3 1. One mole of an ideal gas expands isothermally at T = 20°C from 1.2 m² to 1.8 m². The gas constant is given by R= 8.314 J/mol K). (a) Calculate the work done by the gas during the isothermal expansion. W= (b) Calculate the heat transfered during the expansion Q= (c) What is the change in entropy of the gas? AS аук (c) What is the entropy change of the thermal reservoir? AS reservar JK (d) What is...
Vol calculate mol sample of an ideal gas expands reversibly and isothermally to a final OL If the initial pressure is 7.0 am and the temperature is 57.0°C (a) the initial volume of the gas (b) the final pressure of the gas (c) the work done in kJ (5) A 2 50 mol sample of an ideal monoatomic gas at 300K expands adiabatically and reversibly from a volume of 15.0 L to 60.0L Calculate the (a) final temperature of the...
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?
Extra Credit (20 pts) 10 moles of an ideal gas expands from a volume of 0.2 m3 to a volume of 0.8 m3 by an adiabatic free expansion (no work). a. Does the internal energy of the gas change? Why or why not? b. Does the temperature of the gas change? Why or why not? c. Does the entropy of the gas change? Why or why not d. Would the entropy change be any different if the gas expanded from...
Five moles of an ideal gas expands isothermally at 300 K from an initial volume of 100 L to a final volume of 500 L. Calculate: (a) the maximum work the gas can deliver, (b) the heat accompanying the process, (c) ∆S for the gas. (Please explain why did you use the equation, what conditions did you see from the question, etc)
Five moles of an ideal gas expands isothermally at 300 K from an initial volume of 100 L to a final volume of 500 L. Calculate: (a) the maximum work the gas can deliver, (b) the heat accompanying the process, (c) AS for the gas.
A monatomic ideal gas is initially at volume, pressure, temperature (Vi, Pi, Ti). Consider two different paths for expansion. Path 1: The gas expands quasistatically and isothermally to (Va, Pz. T2) Path 2: First the gas expands quasistatically and adiabatically (V2, P.,T-),where you will calculate P T. Then the gas is heated quasistically at constant volume to (Va. P2 T1). a. Sketch both paths on a P-V diagram. b. Calculate the entropy change of the system along all three segments...
A sample of 70 mmol Kr(g) expands reversibly and isothermally at 373 K from 5.25 cm^3 to 6.29 cm^3, and the internal energy of the sample is known to increase by 83.5 J. For a given expansion, do you expect the heat absorbed by a real gas to be greater than or less than the heat absorbed by an ideal? Explain your answer. Use the virial equation of state up to the second coefficient B = -28.7 cm^3 mol-1 to...