Dalton's Law Partial Pressure and Mole Fraction

A container holds methane gas with a pressure of 0.175 atm and oxygen gas with a pressure of 0.250 atm. What is the total pressure of the gas in the container?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A tank contains a mixture of 52.5 g oxygen gas and 65.1 g carbon dioxide gas at 27^oC. The total pressure in the tank is 9.21 atm. Calculate the partial pressures of each gas in the container.

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A container contains three gases, N₂, O₂ and Ar, with partial pressures of 23.3 kPa, 40.9 kPa and 13.7 kPa respectively. What is the total pressure inside the container?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A mixture of 2 moles of H₂, 3 moles of NH₃, 4 moles of CO₂, and 5 moles of N₂ exert a total pressure of 800 mm Hg. What is the partial pressure of each gas?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A gas mixture contains hydrogen, helium, neon and argon. The total pressure of the mixture is 93.6 kPa. The partial pressures of helium, neon and argon are 15.4 kPa, 25.7 kPa, and 35.6 kPa, respectively. What is the pressure extended by the hydrogen?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A mixture of gases contains 2.14 g of N₂, 5.85 g of H₂, and 4.18 g of NH₃. If the total pressure of the mixture is 4.58 atm, what is the partial pressure of each component?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

A certain reaction occurs, producing an oxide of nitrogen as a gas. The gas has a mass of 1.211 g and occupies a volume of 677 mL. The temperature in the laboratory is 23°C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

The density of a gas is measured at 1.853 g / L at 745.5 mmHg and 23.8 °C. What is its molar mass?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

Aluminum chloride, AlCl₃, sublimes at high temperatures. What density will the vapor have at 225 degrees Celsius and 0.939 atm of pressure?

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation

An elemental gas (meaning that it is made from one element) has a mass of 10.3 grams. It occupies 58.4 L at 1.00 atm and 2.50 °C. Identify the gas.

• Dalton's Law of Partial Pressure

• Graham's Law

• Mole Fraction

• Density equation

• Molar mass equation