Mass of flask, Al foil and Cu wire (g): 90.4576 g Mass of flask, Al foil, Cu wire and condensed vapor (g): 90.8488 Temperature of vapor (℃): 100.5 Volume of flask (mL): 154 Barometric pressure (mmHg): 746.5   Determine the molar mass of the vapor molar mass= mass/moles

A 0.470 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H2SO4 (aq) →MSO4 (aq) + H2(g) A volume of 217 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 \deg C. The vapor pressure of water at 25 \deg C is 23.8 Torr. Calculate the molar mass of the metal.

At 298 K, a 5.0-L flask contains 0.15 mol of O2 and 0.22 mol of N2. Calculate the partial pressure of N2 inside the container. (Note: the ideal gas constant is 0.0821 L•atm/mol•K)

Give typed solution only

1. A 23.1 mL sample of H2 gas was collected from an experiment at 1.079 atm and 22.9  °C. How many moles of gas are in this sample? 2. Suppose you are collecting a gas over water at 23 oC and obtain a pressure reading of 788.3 mm Hg.If the vapor pressure of water is 21.1 mm Hg at the collection temperature, what is the pressure of the collected gas? These are two different questions

At 72.5oC and 1.89 atm, 8.14 g of a hydrocarbon vapor has a volume of 2.26 L. What is the molecular weight in g/mol of the hydrocarbon?

What is the experimental molar mass (that is, calculated from the data given and not taken from the periodic table) of magnesium if 0.0325 grams of magnesium generates 33.02 mL of hydrogen at 23.7 °C with a hydrogen partial pressure of 753.7 torr? Note that the partial pressure of water vapor has already been subtracted from the total pressure. 26.0 g/mol 18.8 g/mol 26.2 g/mol 24.2 g/mol 21.8 g/mol

Using the ideal gas law, determine the temperature of a sample of water in the gas phase with 5.00 moles H2O in a 23.0 L flask at 8.00 atm pressure.