A 4.0 mol sample of O2 gas starts off with a volume of 20 L at...
A 4.0 mol sample of O2 gas starts off with a volume of 20 L at 270 K. It is allowed to undergo an adiabatic expansion against a constant pressure of 600 torr until the volume has increased by a factor of 3. Calculate q, w, ∆T, ∆U, and ∆H, for this process. Note: consider this process carefully. Is it reversible? Is the final pressure 600 torr? Treat the gas as ideal.
Homework Answers
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Assume there's 1 mol ideal mono-atomic gas in a 22.4L container at 300K. The initial entropy...
Assume there's 1 mol ideal mono-atomic gas in a 22.4L container
at 300K. The initial entropy of the system is 100J/K. For the
following processes, calculate:
a) q and w for a reversible expansion to twice the volume,
isothermally.
b)
S and
G for irreversible isothermal expansion against a constant 0.5 bar
external pressure, to a final internal pressure of 0.5 bar.
c)
U and
H for adiabatic reversible expansion to twice the volume.
A sample of 5.0 mol CO2(g) is originally confined in 15 dm3 at 280 K and...
A sample of 5.0 mol CO2(g) is originally confined in 15 dm3 at 280 K and then undergoes adiabatic expansion against a constant pressure of 78.5 kPa until the volume has increased by a factor of 4.0. Calculate q, w, delta T, and delta U, and delta H. (The final pressure of the gas is not necessarily 78.5 kPa.) If the enthalpy you calculate does not equal -4.5 kJ and the temperature change - 24 K, you made a mistake.
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.
A sample of an ideal gas in a cylinder of volume 4.14 L at 298 K...
A sample of an ideal gas in a cylinder of volume 4.14 L at 298 K and 2.24 atm expands to 7.48 L by two different pathways. Path A is an isothermal, reversible expansion. Path B has two steps. In the first step, the gas is cooled at constant volume to 1.38 atm . In the second step, the gas is heated and allowed to expand against a constant external pressure of 1.38 atm until the final volume is 7.48...
A sample of an ideal gas in a cylinder of volume 2.82 L at 298 K...
A sample of an ideal gas in a cylinder of volume 2.82 L at 298 K and 2.63 atm expands to 8.40 L by two different pathways. Path A is an isothermal, reversible expansion. Path B has two steps. In the first step, the gas is cooled at constant volume to 1.40 atm, In the second step, the gas is heated and allowed to expand against a constant external pressure of 1.40 atm until the final volume is 8.40L. Calculate...
For the following processes, calculate the indicated quanti- ties for a system consisting of 1 mol...
For the following processes, calculate the indicated quanti- ties for a system consisting of 1 mol of N2 gas. Assume ideal gas behavior. a. The gas, initially at 10 bar, is expanded tenfold in volume against a constant external pressure of 1 bar, all at 298 K. Calculate q, w, ?U and ?H for the gas. b. After the expansion in part (a), the volume is fixed, and heat is added until the temperature reaches 373 K. Calculate q, w,...
3.1 moles of ideal gas undergo an expansion from V1 = 1.2 m3 to V2 =...
3.1 moles of ideal gas undergo an expansion from V1 = 1.2 m3 to V2 = 1.7 m3 during an isothermal process taking place at T = 25 degree C. Calculate Delta U, Delta H, Q, W when The expansion takes place in The following conditions: A reversible expansion. A rapid non-reversible expansion against a constant surrounding pressure equal to The final pressure of The gas. A free expansion where The gas expands in vacuum against zero external pressure.
5 moles of an ideal gas expand isothermally at T-27°C from an initial volume of 20...
5 moles of an ideal gas expand isothermally at T-27°C from an initial volume of 20 dm3 to a final volume of 60 dm3. Calculate the work for this process for a) expansion against constant external pressure of 105 Pa and b) reversible expansion. 2.
A sample of 1.00 mol perfect gas molecules
A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2 R is put through the following cycle:(a) Constant-volume heating to twice its initial volume,(b) Reversible, adiabatic expansion back to its initial temperature,(c) Reversible isothermal compression back to 1.00 atm. Calculate q, w, ?U, and ?H for each step and overall.
A sample of 1.00 mol of N2 gas is expanded adiabatically from a volume of 10.00...
A sample of 1.00 mol of N2 gas is expanded adiabatically from a volume of 10.00 dm3 and a temperature of 400 K to a volume of 20.00 - 3 -dm3. Assume that nitrogen is ideal, with Cv,m = 5R/2. (i) Find the final temperature if the expansion is carried out reversibly. (ii) Calculate the final temperature if the expansion is carried out with a constant external pressure of 1.00 atm. (iii) Find the final temperature if the gas expands...
Assume there's 1 mol ideal mono-atomic gas in a 22.4L container
at 300K. The initial entropy of the system is 100J/K. For the
following processes, calculate:
a) q and w for a reversible expansion to twice the volume,
isothermally.
b)
S and
G for irreversible isothermal expansion against a constant 0.5 bar
external pressure, to a final internal pressure of 0.5 bar.
c)
U and
H for adiabatic reversible expansion to twice the volume.
A sample of 5.0 mol CO2(g) is originally confined in 15 dm3 at 280 K and then undergoes adiabatic expansion against a constant pressure of 78.5 kPa until the volume has increased by a factor of 4.0. Calculate q, w, delta T, and delta U, and delta H. (The final pressure of the gas is not necessarily 78.5 kPa.) If the enthalpy you calculate does not equal -4.5 kJ and the temperature change - 24 K, you made a mistake.
A sample of an ideal gas in a cylinder of volume 2.82 L at 298 K and 2.63 atm expands to 8.40 L by two different pathways. Path A is an isothermal, reversible expansion. Path B has two steps. In the first step, the gas is cooled at constant volume to 1.40 atm, In the second step, the gas is heated and allowed to expand against a constant external pressure of 1.40 atm until the final volume is 8.40L. Calculate...
3.1 moles of ideal gas undergo an expansion from V1 = 1.2 m3 to V2 = 1.7 m3 during an isothermal process taking place at T = 25 degree C. Calculate Delta U, Delta H, Q, W when The expansion takes place in The following conditions: A reversible expansion. A rapid non-reversible expansion against a constant surrounding pressure equal to The final pressure of The gas. A free expansion where The gas expands in vacuum against zero external pressure.
5 moles of an ideal gas expand isothermally at T-27°C from an initial volume of 20 dm3 to a final volume of 60 dm3. Calculate the work for this process for a) expansion against constant external pressure of 105 Pa and b) reversible expansion. 2.
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