One liter of an ideal monatomic gas (gamma=5/3) at atmospheric pressure (1.0 atm) and a temperature...

One liter of an ideal monatomic gas (gamma=5/3) at atmospheric pressure (1.0 atm) and a temperature of 300K is used in the following cycle: an adiabatic compression to one half its original volume, followed by a constant-volume cooling to 300K, followed by an isothermal expansion back to original volume. Determine the work done by the gas, the heat entering the gas and the change in thermal energy of the gas in each leg of the cycle. Organize answer in table. is this cycle allowed by the second law of thermodynamics? what kind of heat machine does this cycle represent? heat engine? refrigerator? explain

Expert Solution

during adiabatic process T₁V₁^-1 = T₂V₂^-1

T₂ =300*(2)^2/3 = 476.4k

work done in adiabatic process is W = nR / - 1( T₁ - T₂ )

W = $\left [$ 8.314 / 22.4 ( 5/3 -1) $\left \right ]$ ( 300-476.4)

W = -98.2 J

work done in isothermal process W =2.303nRT ( v₂ / v₁ )

W = 77.18J

the heat entering the gas Q = W = 77.18J

this cycle is not allowed the second law of thermodynamics

it is a refrigerator

genius_generous answered 4 months ago

A monatomic ideal gas is at an initial pressure of 1.54 atm and 76.0 cm3. The...

A monatomic ideal gas is at an initial pressure of 1.54 atm and 76.0 cm3. The gas undergoes an isochoric increase in pressure to 2.31 atm, then an isobaric expansion to 114 cm3. Pressure is reduced isochorically to the original pressure before an isobaric compression returns the gas to its initial values. For 1.95 moles of the gas, complete the following: a) Generate a sketch of the PV diagram, with values clearly represented. b) Find the heat absorbed and heat...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.40 atm ; the volume of the gas changes from 3.20×10-2 m3 to 4.50×10−2 m3 . a. Calculate the initial temperature of the gas. b. Calculate the final temperature of the gas. c. Calculate the amount of work the gas does in expanding. d. Calculate the amount of heat added to the gas. e. Calculate the change in internal energy of the gas.

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ;...

Three moles of an ideal monatomic gas expand at a constant pressure of 2.10 atm ; the volume of the gas changes from 3.30×10−2 m3 to 4.50×10−2 m3 . a) Calculate the initial temperature of the gas. b) Calculate the final temperature of the gas. c) Calculate the amount of work the gas does in expanding. d) Calculate the amount of heat added to the gas. e) Calculate the change in internal energy of the gas

An ideal monatomic gas at an initial temperature of 500 K is expanded from 5.0 atm...

An ideal monatomic gas at an initial temperature of 500 K is expanded from 5.0 atm to a final pressure of 1.0 atm. Calculate w, q, DU, and (where applicable) DH and DT when the expansion is performed (a) reversibly and isothermally, and (b) reversibly and adiabatically. Help Please!!!

An ideal gas with 7 degrees of freedom begins at a pressure of 8.5 atm, temperature...

An ideal gas with 7 degrees of freedom begins at a pressure of 8.5 atm, temperature of 25 degrees Celsius and volume of 120L. A) How many moles of gas are there? B) The gas expands isobarically to 200L. What is the new temperature? C) How much work was done in the expansion? D) By how much did the internal energy increase? E) What amount of heat flowed into the gas? G) The gas then depressurizes isochorically to the original...

One mole of an ideal monatomic gas initially at 300 K and a pressure of 15.0...

One mole of an ideal monatomic gas initially at 300 K and a pressure of 15.0 atm expands to a final pressure of 1.00 atm. The expansion can occur via any one of four different paths: a. isothermal and reversible, b. isothermal and irreversible, c. adiabatic and reversible, and d. adiabatic and irreversible. In irreversible processes, the expansion occurs against an external pressure of 1.00 atm. For each case, calculate the values of q, w, DU, and DH. I need...

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm...

3 moles of an ideal gas with 2 atoms under 308 K temperature and 5 atm are expanded reversible to 1 atm end pressure. Calculate w, q, ΔU, ΔH values in case of expansion of this expansion by isothermal and adiabatic way.

A gas occupies a volume of 0.35 m3 at a pressure of 1.0 atm. The pressure...

A gas occupies a volume of 0.35 m3 at a pressure of 1.0 atm. The pressure is increased linearly with respect to volume until a final pressure of 2.0 atm is reached, with the final volume being 0.20 m3 . a. Can you tell from the given information if this gas is an ideal gas? b. Calculate the work done on the gas during the compression.

Helium, a monatomic gas, is initially at a pressure of 15 atm, a volume of 1.1...

Helium, a monatomic gas, is initially at a pressure of 15 atm, a volume of 1.1 L, and a temperature of 588 K. It is quasi-statically expanded at constant temperature until its volume is 3.9 L, and is then quasi-statically compressed at constant pressure until its volume and temperature are such that a quasi-static adiabatic compression will return the gas to its original state. (b) Find the volume and temperature after the compression at constant pressure volume______ L temperature ____...

The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature.

The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature. If the initial volume of the as is 472 mL. what is the final volume of the gas? A 4.00 L sample of gas is cooled from 71 CC to a temperature at which its volume is 2.60 L. What is this new temperature? Assume no change in pressure of the gas. A scuba diver releases a...

Question