Question

The initial state of a 1.00 mol of gass is (P=3.00atm, V=1.00L, and Eint = 456J),...

The initial state of a 1.00 mol of gass is (P=3.00atm, V=1.00L, and Eint = 456J), and its final state is (P = 2.00atm, V= 3.00L and Eint = 912J). the gas is allowed to expand isothermally until it reaches its volume and its pressure is 1.00atm. It is then heated at a constant volume until it reaches its final pressure.

(a) illustrate this process on a PV diagram and calculate the work done by the gas.

(b) find the heat absorbed by the gas during this process.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
The gas is first cooled at constant volume until it reaches its final pressure. It is...
The gas is first cooled at constant volume until it reaches its final pressure. It is then allowed to expand at constant pressure until it reaches its final volume. (Use the following as necessary: P1 = 2.90 atm, V1 = 0.90 L, and Eint 1 = 451 J and its final state P2 = 2.10 atm, V2 = 2.90 L, and Eint 2 = 910 J.) (a) Illustrate this process on a PV diagram (Do this on paper. Your instructor...
A mole of a monatomic ideal gas is taken from an initial pressure p and volume...
A mole of a monatomic ideal gas is taken from an initial pressure p and volume V to a final pressure 3p and volume 3V by two different processes: (I) It expands isothermally until its volume is tripled, and then its pressure is increased at constant volume to the final pressure. (II) It is compressed isothermally until its pressure is tripled, and then its volume is increased at constant pressure to the final volume. Show the path of each process...
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)...
An ideal gas initially at P = 175 torr and V = 2.00 dm3 is allowed...
An ideal gas initially at P = 175 torr and V = 2.00 dm3 is allowed to expand against an external pressur of 122 torr until the pressures are equal. What is the work done by this process? What would be the work done if the gas expanded to the same final volume under an external pressure of 175 torr and was then allowed to relax at constant volume to the final pressure of 122 torr?
n = 2.58 mol of Hydrogen gas is initially at T = 376 K temperature and...
n = 2.58 mol of Hydrogen gas is initially at T = 376 K temperature and pi = 1.88×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 8.78×105 Pa. What is the volume of the gas at the end of the compression process? What would be the temperature of the gas, if the gas was allowed to adiabatically expand back to its original pressure?
The working substance of an engine is 1.00 mol of a monatomic ideal gas. The cycle...
The working substance of an engine is 1.00 mol of a monatomic ideal gas. The cycle begins at P1=1.00 atm and V1=24.6L. The gas is heated at constant volume to P2=2.00atm. It then expands at constant pressure until its volume is 49.2L. The gas is then cooled at constant volume until its pressure is again 1.00 atm. It is then compressed at constant pressure to its original state. All the steps are quasi-static and reversible. Calculate the TOTAL work done...
n = 4.13 mol of Hydrogen gas is initially at T = 367.0 K temperature and...
n = 4.13 mol of Hydrogen gas is initially at T = 367.0 K temperature and pi = 1.85×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 6.59×105 Pa. What is the volume of the gas at the end of the compression process? A. How much work did the external force perform? B. How much heat did the gas emit? C. How much entropy did the gas emit? D. What would be...
n = 4.44 mol of Hydrogen gas is initially at T = 357.0 K temperature and...
n = 4.44 mol of Hydrogen gas is initially at T = 357.0 K temperature and pi = 3.03×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 9.97×105 Pa. a) What is the volume of the gas at the end of the compression process? b) How much work did the external force perform? c) How much heat did the gas emit? d) How much entropy did the gas emit? e) What would...
1- A- n = 4.46 mol of Hydrogen gas is initially at T = 386.0 K...
1- A- n = 4.46 mol of Hydrogen gas is initially at T = 386.0 K temperature and pi = 2.16×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 8.85×105 Pa. What is the volume of the gas at the end of the compression process? B- How much work did the external force perform? C- How much heat did the gas emit? D- How much entropy did the gas emit? E- What...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT