Given a sample of 1.48 g of helium and an unknown mass of O₂ mixed in a flask at room temperature, with the partial pressures of helium and oxygen being 41.2 torr and 159 torr respectively, what is the total pressure in the flask?

A gas mixture with a total pressure of 795 mmHg contains the following gases at the indicated partial pressures: 155 mmHg CO2, 235 mmHg Ar, and 109 mmHg O2. The mixture also contains helium gas. What mass of helium gas is present in the mixture, given that the molar mass of helium is 4.00 g/mol?

A mixture of 10.0 g of Ne and 10.0 g of Ar has a total pressure of 1.60 atm. What is the partial pressure of Ar in the mixture?

A mixture of 7.87 g CH4 and 7.13 g Xe is placed in a container, and the total pressure is found to be 0.51 atm. Determine the partial pressure of Xe in atm.

A mixture of argon and hydrogen gases, in a 6.38 L flask at 90°C, contains 6.37 grams of argon and 0.399 grams of hydrogen. The partial pressure of hydrogen in the flask is ___ atm and the total pressure in the flask is ___ atm. What is the partial pressure of hydrogen in the flask?

What is the total pressure (in atm) inside a vessel containing N2 exerting a partial pressure of 0.256 atm, He exerting a partial pressure of 203 mmHg, and H2 exerting a partial pressure of 39.0 kPa?

If the partial pressure of a gas in a mixture has declined to one third of its initial value, what is the new partial pressure if the initial pressure was 90 kPa?

Which of the following statements about partial pressures of gases in the lungs is true?

Which of the following statements about partial pressures of gases in the tissues is true?