Shown below is a gas sample contained in a cylinder with a movable piston.
The temperature is increased from 200 K to 400 K while the pressure is decreased from 2.6 atm to 1.3 atm. Which of the following images illustrate the gas sample after?
Suppose a gas sample is contained in a cylinder with a movable piston. The Kelvin temperature of the gas is doubled while its volume is reduced by one-third. Identify the change in the pressure of the gas.
Consider a gas in a fixed volume sealed container at 20°C. Which statement below describes a method to reduce the pressure of the gas by half?
i) Increasing the gas temperature up to 40°C
ii) Decreasing the gas temperature up to 10°C
iii) adding the same amount of gas as initially present
A flask contains 16.3 g Xe, 7.52 g Cl2, and 4.15 g He. Calculate the mole fraction of Cl2 in the flask.
A vessel contains CO, H2, and O2. The mole fractions of H2 and O2 are 0.17 and 0.62, respectively. What would be the mole fraction of CO?
0.672 g of SO2 and 1.28 g of Ar at 289 K are both present in an 25.00-L flask. In mmHg, what is the partial pressure of Ar?
The air pressure on top of the world's tallest mountain is 253 mmHg. If the mole fraction of nitrogen gas in air is 0.7808, what is its partial pressure in mmHg at the summit of the mountain?
At 25°C, a 1.00 L vessel is filled with 2.30 g of argon. A sample of ethane vapor was introduced to the same vessel until the total pressure reaches 1.620 atm.
a. Determine the partial pressure of argon (PAr).
b. Determine the partial pressure of ethane (Pethane).
A 250 mL evacuated flask has a mass of 112.78 g when filled with 378 torr of an unknown gas at 29.0 °C. What is the molar mass of the unknown gas if the mass of the 250 mL evacuated flask is 112.36 g?
Xylene is a hydrocarbon used as a gasoline additive. It is made up of 90.5% C and 9.5% H by weight. At 101.325 kPa and 130°C, 2.34 g of xylene occupies a volume of 729.1 mL. Determine the molecular formula of xylene.
The following data for an unknown vapor were obtained through the Dumas-bulb method:
Mass = 0.366 g
Volume = 355 mL
Pressure = 100 kPa
Temperature = 100°C
Determine the molar mass of the unknown vapor.
The air we breathe is composed of different gases. At near sea level (288.15 K), the density of air is approximately 2.7×1019 molecules/cm3. Calculate the air pressure in millimeters of mercury.
A sample of a gas is found to have a density of 1.457 g/L at 34.0 °C and 835 torr. What is the molar mass of the gas?
