Question

Which one has lower final temperature for an adiabatic process, reversible or irreversible, when expanding to...

Which one has lower final temperature for an adiabatic process, reversible or irreversible, when expanding to the same final volume for an ideal gas?

Homework Answers

Answer #1

Since, In case of reversible adiabatic expansion of the ideal gas there will be maximum amount of work done because of no heat loss in extra forces like friction etc. So, the final temperature will be more in case of reversible adiabatic expansion of the ideal gas. On the other hand in case of irreversible adiabatic expansion of the ideal gas there will be heat loss in the extra forces like friction etc. So, the temperature will be less in case of irreversible adiabatic expansion of the ideal gas.

Then the irreversible adiabatic expansion of the ideal gas will have the lower temperature than the reversible adiabatic expansion of the ideal gas.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
One mole of the gas Ar expands through a reversible adiabatic process, from a volume of...
One mole of the gas Ar expands through a reversible adiabatic process, from a volume of 1 L and a temperature of 300 K, to a volume of 5 L. A) what is the final temperature of the gas? B) How much work has the expansion carried out? C) What is the change in heat? Assume this is a mono-atomic ideal gas. Note by asker: as the gas is mono-atomic, cp=(5/2)*R, cv=(3/2)*R
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
I'm having a little bit of difficulty with adiabatic reversible expansions...Concerning this extended problem how do...
I'm having a little bit of difficulty with adiabatic reversible expansions...Concerning this extended problem how do I go about solving it? Q: Consider adiabatic reversible expansion of Neon gas under ideal conditions at 75 kPa. Calculate the expected final state pressure when the gas expands to 3/2 the volume of the initial state. Moreover, consider adiabatic, reversible expansion of 0.10 mol of carbon dioxide behaving as an ideal gas. Calculate the work done by the gas when it expands to...
2. p1V1γ= p2V2γ is only correct when (a) a perfect gas undergoes an adiabatic process.        (b)...
2. p1V1γ= p2V2γ is only correct when (a) a perfect gas undergoes an adiabatic process.        (b) a perfect gas undergoes a reversible process. (c) a perfect gas undergoes a reversible adiabatic process.     (d) a real gas undergoes a reversible adiabatic process.      4. If a simple (meaning one-component, single phase) and homogeneous closed system undergoes an isobaric change with expansion work only, how Gibbs free energy varies with temperature?      (a) (G/T)p> 0        (b) (G/T)p< 0      (c) (G/T)p= 0        (d) Depending on...
Calculate the total change of entropy for an ideal monatomic gas expanding from a volume V...
Calculate the total change of entropy for an ideal monatomic gas expanding from a volume V into a volume 2V via: i) Free expansion ii) Quasi-static isothermal expansion iii) Quasi-static adiabatic expansion; iv) Do the results of (iii) surprise you? Comment on what these results mean in terms of reversible and irreversible processes.
If a perfect gas undergoes adiabatic compression, is the initial temperature lower, higher, or the same...
If a perfect gas undergoes adiabatic compression, is the initial temperature lower, higher, or the same as the final temperature.
Consider the adiabatic, reversible expansion of a closed 1 mole sample of monatomic ideal gas from...
Consider the adiabatic, reversible expansion of a closed 1 mole sample of monatomic ideal gas from P1 = 100 bar, V1 = 1dm3, and T1 = 1200K to V2 = 1.5 dm3. What is the final temperature of the gas? What are the values of ΔE, ΔS and w for the process described in the previous question? ΔE = kJ ΔS = J/K w = kJ
Ideal gas ethylene undergoes a reversible adiabatic compression by which its temperature increases from T1 =...
Ideal gas ethylene undergoes a reversible adiabatic compression by which its temperature increases from T1 = 300 K to T2 = 450 K. The molar entropy in the initial state is given as s1 = 100 J K–1 mol–1, and here, for ethylene, cp = ?T + c0 with ? = 0.1 J K–2 mol–1 and c0 = 13.1 J K–1 mol–1. Determine the change of the molar entropy s2 – s1 and the change of the chemical potential ?2...
select correct option To get a speed of propagation, Newton assumed that the process is (...
select correct option To get a speed of propagation, Newton assumed that the process is ( A ). While he assumed the process is ( A ), which means the temperature is conserved during the process, the speed of propagation is quite different with the real one. Laplace's modified equation considered the process as ( B ), which means the process occurs without the transfer of heat or matter between a system and its surroundings. When the process is (...
2 kilograms of steam at 2000 kpa and 270C undergoes a reversible, adiabatic expansion to a...
2 kilograms of steam at 2000 kpa and 270C undergoes a reversible, adiabatic expansion to a final state at which the steam is a saturated vapor. A) Determine Temperature and pressure of the final state B) Calculate Work, W for the expansion process
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT