Calculate the change in the Hemholtz energy when four moles of an ideal gas at 125 degrees C undergoes an isothermal expansion from 3.75 L to 8.25 L.
This is physical chemistry, please someone help.
Calculate the change in the Hemholtz energy when four moles of an ideal gas at 125...
physical chemistry
3. Derive formulas for AE, Aw, and Aq when a Van der Waal's gas undergoes: a) reversible isothermal expansion b) adiabatic expansion c) repeat steps a and b for an ideal gas d) Use the Maxwell relation derived from the Helmholtz free energy F =F(T,V) = -SdT PdV To prove that e) Determine for a Van der Waal's gas and an ideal gas. T()-P f) Explain the answer to part e in terms of the assumptions that define...
An ideal gas undergoes a reversible isothermal expansion at 57.0 degree C, increasing it's volume from 1.50 L to4.50 L. The entropy change of the gas is 36.0 J/K. How many moles of gas are present?
5. Isothermal (87°C) reversible expansion of 3.00 moles of an ideal gas from 7.00 to 13.00 liters. (Cv.m=(3/2)R a. Calculate AS for the reversible expansion. b. Calculate w (work). c. What are AU and AH, the change in internal energy and change in enthalpy, respectively?
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
400 moles of an ideal monatomic gas are kept in a cylinder fitted with a light frictionless piston. The gas is maintained at the atmospheric pressure. Heat is added to the gas. The gas consequently expands slowly from an initial volume of 10 m3 to 15 m3. (a) Draw a P-V diagram for this process. (b) Is this thermodynamic process an isothermal expansion, an isobaric expansion or an adiabatic expansion? (c) Calculate the work done by the gas. (d) Calculate...
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.
¨Calculate the entropy change when 2 moles of an ideal gas are allowed to expand isothermally from an initial volume of 1.5 L to 2.4 L. Then estimate the probability that the gas will contract spontaneously from the final volume to the initial one.
An ideal gas (1.82 moles) undergoes the following reversible Carnot cycle. (1) An isothermal expansion at Thot=850K from 3.20L to 20.40L. (2) An adiabatic expansion until the temperature falls to 298K. The system then undergoes (3) an isothermal compression and a subsequent (4) adiabatic compression until the initial state is reached. a. Calculate work and ΔS for each step in the cycle and its overall efficiency. b. Determine ΔH and ΔU for steps (1) and (2). c. Explain why ΔUcycle=...
5. Calculate the change in entropy of an ideal gas when 2.00 moles of it is changed from 25 °C and 1.50 atm to 135 °C and 7.00 atm. You may assume that Cp.m=5/2 R. (10 pts) J/K
One mole of an ideal gas undergoes a reversible isothermal expansion from a volume of 1 L to a volume of 2 L. The change in entropy of the gas in terms of the universal gas constant R is? Final Answer is R ln(2), but I need to know how to calculate this