A volume meter operates at 28 °C and an internal vacuum of 24 mm Hg. Barometric pressure is 756 mm Hg. The meter measures 13 ft3 of air. What is the volume at standard ambient conditions?

In a container of 80 I at 50 ° C under vacuum, 7 g of N2, 16 g of O2 and 3.03 g of H2 are introduced. Calculate the partial pressure of each gas, the total pressure, and the composition of the mixture in mole percent.

1.25 L container holds a stoichiometric mixture* of ethene (CaH4), ethane (CaH6) and oxygen at a total pressure of 1.55 atm and a temperature of 24.5 °C. The mixture is ignited and completely combusts to form carbon dioxide and water. The water is removed from the vessel, leaving only carbon dioxide at a total pressure of 0.926 am at the same conditions. What is the mole fraction of oxygen in the original mixture?

A compressed gas cylinder at 13,700 kPa and 23°C, is in a room where a fire raises the temperature to 450.°C. What is the new pressure of the cylinder, in atm? The volume of the cylinder does not change.

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. || atm O

A mixture of gases consists of 0.4 kg of oxygen, 0.7 kg of carbon dioxide, and 0.2 kg of helium. This mixture is maintained at 100 kPa and 27 °C. Determine the apparent molecular weight of this mixture the volume it occupies, the partial volume of the oxygen, and the partial pressure of the helium. (

a cylinder was connected to an open ended U-tube (1 atm) containing some mercury, Hg (density=13.6gcm^-3), and the Hg was displaced 100mm towards the container. What is the pressure of the gas inside the container?