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 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 quantity of 0.27 mole of neon is confined in a container at 2 .50 atm...
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 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 sample of 18 g of oxygen gas (O2) 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 (CP,m) of O2 is 29.355 J mol-1 K-1
Neon gas is heated from 298 K (1 atm pressure) to 500 K under the following conditions: (a) at constant volume; (b) at constant pressure. In each case, find the molar entropy of the gas in its final state (at 500 K) given that its standard molar entropy at 298 K is 146.33 J/mol K. Assume that neon is ideal gas.
Consider a system consisting of 3.0 mol CO2(g), initially at 35°C and 9.0 atm and confined to a cylinder of cross-section 100.0 cm2. The sample is allowed to expand irreversibly and adiabatically against an external pressure of 2.5 atm until the piston has moved outwards through 25 cm. Assume that carbon dioxide may be considered a perfect gas with CV,m = 28.8 J K–1 mol–1, and calculate (a) q, (b) w, (c) ΔU, (d) ΔT, (e) ΔS.
A 2.25 mole sample of carbon dioxide, for which Cp,m= 37.1 JK^-1mol^-1 at 298 K, is expanded reversibly and adiabatically from a volume of 4.50 L and a temperature of 298 K to a final volume of 32.5 L. Calculate the final temperature, q, w,DeltaH and DeltaU. Assume that Cp,m is constant over the temperature interval. (Show all work)
10. (8 points)A 2.00 L container holds 1.12 grams of neon gas and 2.15 grams of krypton gas at a temperature of 298 K. Calculate the total pressure (in atm) of the mixture.
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
Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0L. 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 1.50 atm to a volume of 16.0L. 2. From the end point of step 1,...
A 1.00 mole sample of an ideal monatomic gas, originally at a pressure of 1.00 atm, undergoes, undergoes a three-step process. (1) It is expanded adiabatically from T1 = 550 K, to T2 = 389 K; (2) it is compressed at constant pressure until the temperature reaches T3; (3) it then returns to its original temperature and pressure by a constant volume process. (a) Plot these processes on a PV diagram. (b) Determine T3. (c) Calculate the change in internal energy, the...