Consider 2.0 moles of N2 gas that undergo a reversible isothermal expansion at 250 K from...
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.
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Consider 2.0 moles of N2 gas that undergo a reversible
isothermal expansion at 250 K from...
5. Isothermal (87°C) reversible expansion of 3.00 moles of an ideal gas from 7.00 to 13.00...
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?
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...
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.
Three moles of an ideal gas undergo a reversible isothermal compression at 22.0 ∘C. During this...
Three moles of an ideal gas undergo a reversible isothermal compression at 22.0 ∘C. During this compression, 1700 J of work is done on the gas. Q: What is the change in entropy of the gas? (J/K)
Three moles of an ideal gas undergo a reversible isothermal compression at temperature 17.0 degree C....
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 a reversible isothermal expansion of a gas at temperature τ from volume V to volume...
Consider a reversible isothermal expansion of a gas at temperature τ from volume V to volume V + ∆V . This is not a monatomic ideal gas, but the internal energy of the gas is given by U(τ, V ) = a*V* τ^ 4 , where a is a constant. The pressure is p = (1/3 U)/V . (a) What is the change of energy of the gas in the expansion? (b) How much work is done on the gas...
Consider a reversible adiabatic expansion of 1.00 mol of an ideal gas, starting from 1.90 L...
Consider a reversible adiabatic expansion of 1.00 mol of an ideal gas, starting from 1.90 L and 415 K , if 2.0 kJ of work is done by the expansion. The molar heat capacity at constant volume of the gas is 2.5R. R = 8.314 JK−1mol−1. Determine the final temperature of the gas in the process. Determine the final volume of the gas in the process. Determine the final pressure of the gas in the process.
Two moles of an ideal gas undergo an isothermal expansion at 565 K from a pressure...
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.
640 g of oxygen gas, O2, ondergo reversible isothermal expansion at 35°C from a volume of...
640 g of oxygen gas, O2, ondergo reversible isothermal expansion at 35°C from a volume of 2.4 to 17.3 m. Assuming ideal gas behaviour, what is the total work performed by the gas? A particular reaction has a standard molar reaction enthalpy of -4362 kJ mol" and a standard molar reaction entropy of +21.6 J K-1 mol- both at 298 K. What is the thermodynamic equilibrium constant for the reaction at 298 K? (Note, rounding errors will have a profound...
An ideal gas undergoes a reversible isothermal expansion at 57.0 degree C, increasing it's volume from...
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?
Consider a reversible isothermal expansion of an ideal gas (step 1 in the Carnot cycle). 1.0...
Consider a reversible isothermal expansion of an ideal gas (step 1 in the Carnot cycle). 1.0 mol of ideal gas with Cv =3/2R expands from 2.5L to 10.0L at a temperature (Thot) of 600K. For this process, a) Compute deltaU and deltaH b) Compute w c) Compute q d) Compute delta S Thank you!
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?
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?
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.
640 g of oxygen gas, O2, ondergo reversible isothermal expansion at 35°C from a volume of 2.4 to 17.3 m. Assuming ideal gas behaviour, what is the total work performed by the gas? A particular reaction has a standard molar reaction enthalpy of -4362 kJ mol" and a standard molar reaction entropy of +21.6 J K-1 mol- both at 298 K. What is the thermodynamic equilibrium constant for the reaction at 298 K? (Note, rounding errors will have a profound...
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?
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