Question

Five moles of nitrogen (γ = 1.4) are compressed adiabatically from an initial pressure of 1...

Five moles of nitrogen (γ = 1.4) are compressed adiabatically from an initial pressure of 1 atmosphere and a temperature of 20 ° C to one tenth of its initial volume. Calculate the work and the final pressure of the gas. What is the relationship of the final and initial temperatures?

Homework Answers

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
28g of Nitrogen at STP are adiabatically compressed to a pressure of 25atm. what is final...
28g of Nitrogen at STP are adiabatically compressed to a pressure of 25atm. what is final temperature? what is work done on the gas? what is heat input to the gas? what is the compression ratio? (Vmax/Vmin)
An ideal gas with γ = 1.400 expands adiabatically from a pressure of 365.0 Pa and...
An ideal gas with γ = 1.400 expands adiabatically from a pressure of 365.0 Pa and a volume of 70.00 m3 , doing 101.0 J of work while expanding to a final volume. What is its final pressure-volume product?
An ideal gas with γ=1.4 occupies 5.0 L at 300 K and 120 kPa pressure and...
An ideal gas with γ=1.4 occupies 5.0 L at 300 K and 120 kPa pressure and is heated at constant volume until its pressure has doubled. It's then compressed adiabatically until its volume is one-fourth its original value, then cooled at constant volume to 300 K , and finally allowed to expand isothermally to its original state. Find the net work done on the gas. W= ___J
An ideal gas with ?=1.4 occupies 3.0L at 300 Kand 100kPa pressure and is compressed adiabatically...
An ideal gas with ?=1.4 occupies 3.0L at 300 Kand 100kPa pressure and is compressed adiabatically until its volume is 2.0 L. It's then cooled at constant pressure until it reaches 300 K, then allowed to expand isothermally back to stateA. Find the net work done on the gas and Vmin?
An ideal gas with γ = 1.4 occupies 6.0 L at 300 K and 100 kPa...
An ideal gas with γ = 1.4 occupies 6.0 L at 300 K and 100 kPa pressure. It is compressed adiabatically until its volume is 2.0 L. It's then cooled at constant pressure until it reaches 300 K, then allowed to expand isothermally back to its initial state. a.) Find the net work done on the gas. b.) Find the minimum volume reached.
A volume of O2 is adiabatically compressed from 〖"of " V〗_1=2L to V_2=1L" " and a...
A volume of O2 is adiabatically compressed from 〖"of " V〗_1=2L to V_2=1L" " and a final pressure of 〖 P〗_2="100kPa" . Calculate: (a) the initial pressure, (b) the work, and (c) the variation of kinetic energy
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...
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?
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.