3.1 moles of ideal gas undergo an expansion from V1 = 1.2 m3 to V2 =...
Two moles of an ideal gas undergo a reversible isothermal expansion from 2.41×10−2 m3 to 4.42×10−2 m3 at a temperature of 26.7 ∘C. What is the change in entropy ΔS of the gas? Express your answer numerically in joules per kelvin.
Part A:See diagram 4. 51.4 moles of a diatomic ideal gas undergo three steps: A to B is an isobaric (constant pressure P1 = 5.64x106 Pascal) expansion from volume V1 = 0.0854 m3 to V2 = 0.979 m3. B to C is isochoric (constant volume) C to A is isothermal (constant T). Find PC, the pressure at point C, in Pascals. Express in scientific notation. Part B:See diagram 4. 21.6 moles of a diatomic ideal gas undergo three steps: A...
Two moles of an ideal gas undergo an isothermal expansion at 565 K from a pressure of 12.5 Bar to a final pressure of 1.50 Bar. Calculate AU, AH, and AS for the process if Cy = R. The same ideal gas undergoes an adiabatic expansion from the same initial pressure to the same final pressure (and the same initial temperature). Calculate the final temperature, AU, AH, and AS for the process.
See diagram 4. 22.8 moles of a diatomic ideal gas undergo three steps: A to B is an isobaric (constant pressure P1 = 5.25x106 Pascal) expansion from volume V1 = 0.0248 m3 to V2 = 0.956 m3. B to C is isochoric (constant volume) C to A is isothermal (constant T). During the isobaric expansion from A to B: find Q, the heat transferred, in Joules. Give your answer in scientific notation. NOTE: A positive sign means heat has been...
During a reversible isothermal expansion from volume V1 to volume V2, the work W done by a mole of ideal gas can is: W = RT In () W = 31T in (6) V1 W = RT In 1 V2 W = 34T In ()
Derive) A) the work done by n moles an ideal gas at temperature T in an isothermal expansion from V1 to V2 B) The entropy change of n moles of an ideal gas at Temperature T undergoing an isothermal expansion from V1 to V2
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the volume is doubled in the process. Find q, w, Delta H and the final pressure and temperature for a) reversible adiabatic expansion b) reversible isothermal expansion c) reversible constant pressure expansion d) irreversible adiabat against 0.500 atm external pressure
Three moles of an ideal gas undergo a reversible isothermal compression at temperature 17.0 degree C. During this compression, an amount of work totalling 1600 J is done on the gas. What is the change of entropy of the gas? What is the change of entropy of the gass?
Consider 2.0 moles of N2 gas that undergo a reversible isothermal expansion at 250 K from 3.0 L to 5.0 L. Assume that the gas can be treated as ideal and that it has CV = 5R/2 and a molar mass of 28.01 g/mol. (a). (12 points) Calculate, in kJ/mol, the work, heat, internal energy change, and enthalpy change for the gas. Be sure to show all of your work, including units.
5) Two ideal gas systems undergo reversible expansion under different conditions starting from the same P and V. At the end of the expansion, the two systems have the same volume. The pressure in the system that has undergone adiabatic expansion is lower than in the system that has undergone isothermal expansion. Explain this result without using equations.