A sample of 18 g of oxygen gas (O_{2}) is confined in a container at 200 kPa and 273 K. The gas is allowed to expand adiabatically and reversibly to 100 kPa. Calculate the final temperature of the gas. The molar heat capacity at constant pressure (C_{P,m}) of O_{2} is 29.355 J mol^{-1} K^{-1}
A sample of 18 g of oxygen gas (O2) is confined in a container at 200 kPa and 273 K.
A sample consisting of 65.0 g of xenon is confined in a container at 2.00 atm and 298 K and then allowed to expand adiabatically (a) reversibly to 1.00 atm, (b) against a constant pressure of 1.00 atm. Calculate the final temperature and the expansion work at each case. Use the fact that xenon is a monoatomic gas.
A quantity of neon, confined in a container at 2.50 atm and 298 K, is allowed to expand reversibly and adiabatically satisfying the relation to a final pressure of 1.0 atm. Find the final temperature of the gas. (A) 107 K (B) 207 K (C) 407 K (D) 103 K (E) 241 K
a quantity of 0.27 mole of neon is confined in a container at 2 .50 atm and 298 K and then allowed to expand adiabatically under two different conditions: (a) reversibly to 1.00 atm and (b) against a constant pressure at 1.00 atm calculate the final temperature in each case.
A gas is confined in a container with flexible walls, like a balloon. At 273 K and 5 atm of pressure, the volume of the gas is 10.0 L. If the pressure remains constant while the temperature decreases to 250 K, you would expect the volume of the gas to _____. Increase Vary Widely Remain Constanst Decrease
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...
48 g of methane (CH4) gas is heated reversibly from 200 K to 1800 K at constant pressure conditions. The constant-pressure molar heat capacity of CH4 from 200 K to 1800 K is given by: Cp, molar (T) a + bT + cT-2 where a, b, and c, are constants For CH4, these constants these constants have the values a = JK2 mol, and c =1.825x104 JKmol -1. 31.50 JKmol -1, b 3.824 x10 Calculate the value of AH (in...
A sample of 1.3 mol of CO2 (g) is placed in a 5.0 L rigid container at an initial temperature is 300 K. When 6.98 kJ of heat is added to the system (at constant volume), the temperature rises to 353 K. Calculate q, w, ∆U, ∆H, and CV. The molar heat capacity of O2(g) at constant pressure, is 31.2 J/(K mol) around room temperature. 2.5 mol of O2(g) is heated at constant pressure from 265 K to 310 K....
At 273 K, 1.00 mol of an ideal gas confined to a 2.00-L container exerts a pressure of 11.2 atm. Under the same conditions, what pressure is exerted by CO2, for which a = 3.59 L2 atm mol-2 and b = 0.0427 L mol-1 0 -0.90 10.5 09.1 O 7.2 11.4
A 2.00 mol sample of an ideal gas with a molar specific heat of CV = 5 2 R always starts at pressure 1.50 ✕ 105 Pa and temperature 250 K. For each of the following processes, determine the final pressure (Pf, in kPa), the final volume (Vf, in L), the final temperature (Tf, in K), the change in internal energy of the gas (ΔEint, in J), the energy added to the gas by heat (Q, in J), and the...
A rigid container initially contains 0.6 kg of oxygen at 4,000 kPa and 300 K, the gas cools by lowering the pressure to 3,200 kPa. Determine: (a) the volume of the reservoir, in m3; (b) the final temperature, in K and (c) the total heat transferred, in kJ. That's all I have.