Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of hydrogen, H2, in a 0.50 L flask at 10°C. Assume ideal gas behavior. Given that R = 0.0821 L'atm/(mol-K). O a. 0.279 atm. O b. 0.465 atm. c. 0.349 atm. O d. 0.697 atm. O e. 1.39 atm.

Consider a gas mixture composed of 0.200 mol N2, 0.0800 mol O2, and 0.0200 mol Ar.  The total pressure exerted by this mixture at 25°C is 1.068 atm.  Determine the partial pressure (in atm) of N2 in this mixture.

A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a total pressure of 307.2 kPa. What is the partial pressure of each component of this gas? (The percentages given indicatethe percent of the total pressure that is due to each component.)

A mixture of cyclopropane gas (C3H6) and Oxygen (O2) in a 1.00 to 4.00 mole ratio is used as an anesthetic. What mass of cyclopropane gas is present in a 2.00 L flask at 23.5°C if the total pressure of the oxygen and propane is 1.00 atm? (The molar mass of C3H6 is 42.08 g/mol). A. 8.73 g B. 3.45 g C. 0.69 g D. 2.76 g E. 6.83 mg

14. In a mixture of 2.15 mol of gas, 0.85 mol are nitrogen (N2) molecules. What is the mole fraction of N2 in this mixture? 15. A gas mixture contains 0.150 mol of oxygen (O2) gas and 0.211 mol of argon (Ar) gas. The total pressure of the mixture is 159 kPa. What is the partial pressure of Ar in the mixture?

A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the storage unit rises to 76 °C, causing the gas to decompose and doubling the number of moles in the cylinder. Note: R = 0.08206 Latm/molK Determine the moles of gas in the cylinder before any decomposition occurs. Determine the pressure in the cylinder after the decomposition in atmospheres.

What is the mole fraction of Ne in a gas mixture that contains 0.349 mol Ne and 0.529 mol total? XNe = ___

A 7.00 L tank at 29.4 °C is filled with 2.63 g of sulfur hexafluoride gas and 12.9 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur hexafluoride boron trifluoride mole fraction 0 0 X 00- Ar

One of the major pollutants in the atmosphere has a mass 4.65 x 10-17 gram. If the pressure of the atmosphere is 1.00 Atm, the volume of the air is 4.06 x 10-17 L, and the temperature is 25 oC, use the ideal gas law to identify this gas.

How many moles of gas are in a container that has a volume of 20.5mL, temperature of 303K, and pressure of 1.10atm? Assume ideal gas behavior. Use R=0.08206L atmmol K or 8.314L kPamol K for the ideal gas constant. Your answer should have three significant figures.