Question

For each case determine the change in entropy for the surroundings and the universe, when 1...

For each case determine the change in entropy for the surroundings and the universe, when 1 mole of a diatomic gas expands from its initial volume of 5 L and 31.5 ◦C to:

CASE (a) a final volume of 25 L reversibly and isothermically.

CASE (b) irreversibly and isothermically against an external pressure of 1 atm.

CASE (c) a final volume of 25 L reversibly and adiabatically. Yes, it is zero, but you have to demonstrate it.

CASE (d) irreversibly and adiabatically against an external pressure of 1 atm.

PLEASE, complete answers from CASE A to D.

Science   Advanced-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
A two mole sample of an ideal diatomic gas expands slowly and adiabatically from a pressure...
A two mole sample of an ideal diatomic gas expands slowly and adiabatically from a pressure of 5 atm. and a volume of 10 liters up to a final volume of 30 liters. a) What is the final pressure of the gas ?, b) Whatis the heat, work and internal energy?
One mole of an ideal gas does 3000 J of work on its surroundings as it...
One mole of an ideal gas does 3000 J of work on its surroundings as it expands isothermally to a final pressure of 1.00 atm and volume of 25.0 L. Determine: a) the initial volume ? b) the temperature of the gas? (Note: 1 atm = 1.01 x 105Pa, universal gas constant R = 8.31 J/mol K, 1 L = 10-3m3)
Calculate the change in entropy for one mole of ideal gas which expands from an initial...
Calculate the change in entropy for one mole of ideal gas which expands from an initial volume of 2 L and initial temperature of 500 K to a final volume of 6 L under the following conditions. P(initial) refers to the pressure when T(initial)= 500K, V(initial)= 2 L. a) Irreversible expansion against a constant pressure of Pinitial/2 b) Irreversible expansion against a vacuum...a 'free expansion'. c) Adiabatic irreversible expansion against a constant pressure of Pfinal d) Adiabatic reversible expansion
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...
calculate the molar entropy change when (a) water and (b) benzene are evaporated at their boiling...
calculate the molar entropy change when (a) water and (b) benzene are evaporated at their boiling points at a pressure of 1 atm. what are the entropy changes in (i) the system, (ii) the surroundings, and (iii) the universe, in each case?
Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0...
Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w=____J Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 5.00 atm to a volume of 4.00 L 2. From there, let the...
for the following processes, state whether each of the thermodynamics quantities, q, w, delta U, and...
for the following processes, state whether each of the thermodynamics quantities, q, w, delta U, and delta H is greater than, equal to, or less than zero for the system described. Explain your answers briefly a) an ideal gas expands adiabaticalally against an external pressure of 1 bar. b) an ideal gas expands isothermally against an external pressure of 1 bar c) an ideal gas expands adiabatically into a vacuum d) a liquid at its boiling point is converted reversibly...
A cylinder with a moving piston expands from an initial volume of 0.250 L against an...
A cylinder with a moving piston expands from an initial volume of 0.250 L against an external pressure of 1.00 atm . The expansion does 277 J of work on the surroundings. What is the final volume of the cylinder?
The volume of an ideal gas is adiabatically reduced from 200 L to 74.3 L. The...
The volume of an ideal gas is adiabatically reduced from 200 L to 74.3 L. The initial pressure and temperature are 1.00 atm and 300 K. The final pressure is 4.00 atm. ? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1 atm = 1.013 × 10^5 Pa. mol.K (a) Is the gas monatomic or diatomic? (b) What is the final temperature? (c) How many moles are in the gas?
1 mole of ideal gas at 270C is expanded isothermally from an initial pressure of 3...
1 mole of ideal gas at 270C is expanded isothermally from an initial pressure of 3 atm to afinal pressure of 1 atm in two ways: (a) reversibly and (b) against a constant external pressure of 1 atm. Calculate q, w, ΔU, ΔH and ΔS for each path.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT