A sample of carbon monoxide at 57oC and under 0.67 atm of pressure takes up 85.3 L of space.  What mass of carbon monoxide is present in the sample? (R = 0.0821 Latm/molk)

In Dalton's Law of Partial Pressures: Ptrapped gas = Pdry gas + Pwater vapor  Why must the pressure of water vapor be included in this calculation? a. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. b. Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. c. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor.

A.) a mixture of argon and neon gases, in a 8.32 L flask at 21 degrees Celsius, contains 15.3 grams of argon and 2.24 grams of neon. The partial pressure of neon in the flask is ____atm and the total pressure in the flask is ____atm. B.) a mixture of helium and xenon gases is maintained in a 9.17 L flask at a pressure of 1.28 atm and a temperature of 84 degrees Celsius. If the gas mixture contains 0.637 grams of helium, the number of grams of xenon in the mixture is ____grams.

If 316 mL nitrogen is combined with 178 mL oxygen, what volume of N2O is produced at constant temperature and pressure if the reaction proceeds to 82.0% yield? 2N2​(g)+O2​(g) -----> 2N2​O(g)

If 95 grams of propane is burned during a fire, what volume of carbon dioxide is formed at STP?  C3H8 + O2 --> CO2 + H2O

A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)

SO2 (0.0780mol) and CO2 (0.114mol) are placed in a 750.mL container at 50.0˚C. What is the partial pressure of CO2 in atm?

You have a compound that is 79.9% C and 20.1% H by mass. b. If 3.68 g of the compound is turned to gas in a 2.50 L container at 100°C and 1.50 atm pressure, what is the molecular formula?