14 g of nitrogen gas at STP are adiabatically compressed to a pressure of 25 atm .
What is the final temperature?
What is the work done on the gas?
What is the heat input to the gas?
What is the compression ratio Vmax/ Vmin?
14 g of nitrogen gas at STP are adiabatically compressed to a pressure of 25 atm...
An ideal diatomic gas in a cylinder at 1 atm and 300 K is adiabatically compressed to 1/10th its original volume. What is the final T? How much work was done in the gas to compress it? Why would there be a difference in the computations if the ideal gas were monatomic?
4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and 25°C. Calculate the maximum work (in joules) that can be obtained when the gas is allowed to expand reversibly to a pressure of 1 bar; (a) (10pts) isothermally (b) (15pts) adiabatically The molar heat apacity of nitrogen at constant volume is 20.8 J/K mol. Assume that nitrogen behaves as an ideal gas
4. (25pts) 20L nitrogen gas is compressed in a tank at 10 bar and...
The ideal gas initially at 500 K and 1 atm was compressed adiabatically under two conditions to 5 atm pressure. The final temperature (Ti) under reversible condition and the final temperature (T2) under irreversible condition are related by: O Ti > T2 O T = T2 OT <T2
A. 15.0 mL of nitrogen gas at 0.976 atm is compressed to a pressure of 1.18 atm. What is the new volume? B. What is the pressure in 50.0 L gas cylinder that contains 5.50 grams of nitrogen, N2, at 25oC?
Nitrogen gas is compressed adiabatically in a steady-flow, steady-state process from 0.1 MPa and 25oC at a rate of 0.2 kg/s. The air exits the compression at a temperature of 125oC. Assuming cold-air constant properties, use the values found in Table A-2(a) and determine the exit pressure [kPa] by using the polytropic relationship using n=k.
An ideal gas is compressed isothermally from 8.07 L to 6.35 L, at a starting pressure of 0.467 atm and temperature of 78.00 °C. 1. How many moles of gas are present? Tries 0/3 2. What is the final pressure (in atm) of the gas? Tries 0/3 3. If the compression is carried out reversibly and isothermally, how much work (in J) is done on the system? Tries 0/3 4. What is the heat flow in part 3? Remember that...
A monatomic ideal gas that is initially at a pressure of 1.54 times 10^5 Pa and with a volume of 8.00 times 10^-2 m^3 is compressed adiabatically to a volume of 3.90 times 10^-2 m^3. What is the final pressure? P = ______ Pa How much work is done by the gas during the compression? W = ________ J What is the ratio of the final temperature of the gas to its initial temperature?
1.00-mol sample of N2 gas at 20.09C and 5.00 atm is allowed to expand adiabatically and quasi- C. After it reaches a temperature of 20.09C, it is heated at constant volume until its pressure 72..A stati cally until its pressure equals 1.00 atm. It is then heated at constant pressure until its temperature is is again 5.00 (a) Construct a PV diagram showing each process in the cycle. (b) From your graph, determine the work done by the gas during...
If 2.6m3 of a gas initially at STP is compressed to 1.2m3 and its temperature is raised to 40?C, what is its final pressure? (answer in atm)
A monatomic ideal gas (γ =1.67) is compressed adiabatically to one-twentieth its initial volume with P1 = 1.00 atm. What is the final pressure? Assuming T1=300K, What is T2(final temperature)?