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 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.
An ideal gas, initially at a pressure of 9.1 atm and a temperature of 311 K, is allowed to expand adiabatically until its volume doubles.What is the gas’s final pressure, in atmospheres, if the gas is diatomic?
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.
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
Container A holds 757 mL of ideal gas at 2.50 atm. Container B holds 174 mL of ideal gas at 4.10 atm . If the gases are allowed to mix together, what is the partial pressure of each gas in the total volume?
Suppose 1.50 m^3 of a gas with = 1.40, initially at 300 K and 1.0 atm, is suddenly compressed adiabatically to one half of its initial volume. (1 atm = 101.3 kPa). Find its final pressure final temperature
3) The temperature of an ideal gas confined in a 5 L container is raised from 20 °C to 70 °C. If the initial pressure of the gas was 1.5 atm, what is the final pressure of the gas?