At 0 degrees C, a 1.0-L flask contains 5.0×10−2 mol N2, 1.5×102 mg O2, and 5.0×1021 molecules of NH3. What is the partial pressure of each gas, and what is the total pressure in the flask?

What height of water (in meters) is necessary to measure a pressure of 760 mm Hg? The density of mercury is 13.79 g/cm3, and the density of water is 1.00 g/cm3.

Consider the reaction, 2 Al (s) + 6 HCI (aq) → 2 AICI, (aq) + 3 H, (g). When 40.0 g of Al react with an excess of HCl at 25.0 °C the pressure in a collection flask is measured to be 1.50 atm. What is the volume of the collection flask?

A mixture of gases contains 4.25 grams of CO2 and 2.25 grams of CH4 and has a total pressure of 0.900 atm. What is the partial pressure of CH4?

10. A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.

CO2 was added to a cylinder containing 2.5 atm of O2 to give a total pressure of 4.0 atm of gas. What is the partial pressure of O2 and CO2 in the final mixture?

[5] Sodium chlorate decomposes on heating to sodium chloride and oxygen gas. heat 2NACIO:(s) → 2NaCI(s) + 302(g) A 0.8765 g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 ml at a temperature of 22 °C and a pressure of 734 torr. Calculate the mass percent of NaCIO3 in the original sample. (At 22 °C the vapor pressure of water is 19.8 torr.)

9. a) You have determined experimentally that at standard temperature and pressure (0 °C and 1 atm) that you have a gas weighing 0.1977 g in a 100 mL sealed container. What is the molecular weight of the unknown gas?

A sample of nitrogen gas has a volume of 167.0 mL at STP. What volume (in mL) does the gas occupy if the temperature is increased by 55.3 ºC and the pressure is doubled? 200.0 mL of 3.96 M hydrochloric acid is added to 100.0 mL of 4.60 M barium hydroxide. After the reaction goes to completion, what is the concentration (in mol/L) of the excess H+(aq) or OH–(aq) that remains in solution? Assume that the volumes are additive. Aqueous solutions of the following reactants are mixed. After the reaction goes to completion, calculate the concentration (in mol/L) of silver ions in solution. 160.0 mL of 3.50 M AgNO3 are mixed with 150.0 mL of 1.50 M CaCl2. Consider the following reaction: 2 NH3 (g)   +   3 Cl2 (g)   →   N2 (g)   +   6 HCl (g) A mixture is prepared from 15.0 mol of ammonia and 15.0 mol of chlorine gas. Determine the total moles of gas in the container after the reaction has gone to completion.

1. What is the mole fraction of each gas in a mixture having the partial pressures of 0.467 atm of He, 0.317 atm of Ar, and 0.277 atm of Xe?