Question

1. A diatomic gas (γγ = 1.4) initially in a state with P0, V0, and T0...

1.

A diatomic gas (γγ = 1.4) initially in a state with P0, V0, and T0 undergoes two consecutive processes. During the first, isochoric, process the pressure increases 3.6 times, then the gas expands adiabatically to the initial pressure P0. If the initial temperature T0 = -5°C, find the final temperature of the gas.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

#Hi, if you are happy and find this useful please thumbs up. In case, if you have any query regarding the solution please let me know in the comments section below. We can discuss. Thanks!!

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
One mole of an ideal gas initially at temperature T0 reversibly expands from volume V0 to...
One mole of an ideal gas initially at temperature T0 reversibly expands from volume V0 to 2V0, (a) at constant temperature (b) at constant pressure. Calculate the work, the heat, and change in internal energy of the gas in each process.
A 2.00-mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of...
A 2.00-mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of 5.04 atm and a volume of 13.0 L to a final volume of 31.0 L. (a) What is the final pressure of the gas? atm (b) What are the initial and final temperatures? initial K final K (c) Find Q for the gas during this process. kJ (d) Find ΔEint for the gas during this process. kJ (e) Find W for the gas during...
2.50 mol of a diatomic ideal gas expands adiabatically and quasi-statically. The initial temperature of the...
2.50 mol of a diatomic ideal gas expands adiabatically and quasi-statically. The initial temperature of the gas is 325 K. The work done by the gas during expansion is 7.50 kJ. (a) What is the final temperature of the gas? K (b) Compare your result to the result you would get if the gas were monatomic. (Calculate the final temperature if the gas were monatomic.) K
A 1.79 mol diatomic gas initially at 274 K undergoes this cycle: It is (1) heated...
A 1.79 mol diatomic gas initially at 274 K undergoes this cycle: It is (1) heated at constant volume to 707 K, (2) then allowed to expand isothermally to its initial pressure, (3) then compressed at constant pressure to its initial state. Assuming the gas molecules neither rotate nor oscillate, find (a) the net energy transferred as heat to the gas (excluding energy transferred as heat out of the gas), (b) the net work done by the gas, and (c)...
A 3.44 mol diatomic gas initially at 346 K undergoes this cycle: It is (1) heated...
A 3.44 mol diatomic gas initially at 346 K undergoes this cycle: It is (1) heated at constant volume to 909 K, (2) then allowed to expand isothermally to its initial pressure, (3) then compressed at constant pressure to its initial state. Assuming the gas molecules neither rotate nor oscillate, find (a) the net energy transferred as heat to the gas (excluding energy transferred as heat out of the gas), (b) the net work done by the gas, and (c)...
A 0.50 L container is initially filled with Nitrogen gas at STP. The gas expands against...
A 0.50 L container is initially filled with Nitrogen gas at STP. The gas expands against a piston adiabatically to a volume of 50.0% larger than the original volume. The Nitrogen may be treated as an ideal gas with ?=7/5. a) Calculate the final temperature and pressure. b) What is the work done? c) Sketch a pV-diagram for this process. On this diagram also draw the isotherms for the initial and final temperatures.
Initially 5.00 mol of neon gas (CV = 3R/2 and γ = 5R/2) are at absolute...
Initially 5.00 mol of neon gas (CV = 3R/2 and γ = 5R/2) are at absolute temperature 305 K and occupy volume 4.00×10−2m3. Then the gas expands adiabatically to a new volume of 9.00×10−2m3. A) Calculate the initial pressure of the gas. B) Calculate the final pressure of the gas. C) Calculate the final temperature of the gas. D) Calculate the work done as the gas expands.
3.0 moles of an ideal gas are subjected to the following processes. First the volume is...
3.0 moles of an ideal gas are subjected to the following processes. First the volume is tripled in an isobaric process. Then it undergoes an isothermal process to a pressure of 9.0 kPa. The volume is then cut in half in another isobaric process after being tripled. Finally, it returns to the original state in an isochoric process. (a) Draw a PV diagram of the cycle. Label each state (vertex) with a letter (A, B, …) and each transition with...
4. Three moles of a monatomic ideal gas are initially at a pressure of 1.00 atm...
4. Three moles of a monatomic ideal gas are initially at a pressure of 1.00 atm and a temperature of 20.0OC. The gas is compressed adiabatically to a final pressure of 5.00 atm. Find: (a) the initial volume of the gas; (b) the final volume of the gas; (c) the final temperature of the gas; (d) the work done by the gas during the compression. Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8 atm-L Please show...
a machinr carries 2 moles of an ideal diatomic gas thay is initially at a volume...
a machinr carries 2 moles of an ideal diatomic gas thay is initially at a volume of 0.020 m^3 and a temperature of 37 C is heated to a constant volumes at the temperature of 277 C is allowed to expand isothermally at the initial pressure, and finally it is compressed isobarically to its original volume, pressure and temperature. 1. determine the amount of heat entering the system during the cycle. 2. calculate the net work affected by the gas...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT