Saved cept- Calculate mass of Mg to produce hydrogen gas Magnesium metal is reacted with hydrochloric acid to produce hydrogen gas. A sample of hydrogen gas is collected over water in a eudiometer. Calculate the mass (in grams) of magnesium metal needed to produce 41.0 mL of hydrogen gas at an atmospheric pressure of 739 mmHg and a temperature of 25.9°C. Water Vapor Temperature Pressure (8Huu) 22 19.8 24 22.4 Mass of Mg = %3D 25.2 28 28.3 31.8 30 < Prev 2 of 4 NAxt > 08 F8 F6

Calculate the volume occupied by 25.8 g of methane gas (CH4) at 28°C and 1.0 atm (R = 0.0821 L·atm·K-1·mol-1). 0.039 L 8.7 L 39.8 L 99.2 L 59.7 L

00 96 %24 4. 2 3. 1. %23 L V atm October 12, 1979. Convert this value to atmospheres. The lowest atmospheric pressure ever measured is 652.5 mm Hg, recorded during Typhoon Tip on

A sample of argon gas initially occupies a volume of 30.0 L at a temperature of 25 °C and a pressure of 2.60 atm. Calculate the sample’s temperature (in °C) after the volume of the sample increases to 221 L and its pressure is decreased to 0.50 atm. (Show Work)

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

The height of Mt. Everest is 29,000' and the atmospheric pressure is 253 mmHg (0.333 atm). The gas constant R is 8.314J/K*mol and the heat of vaporization of water (AHvap) is 40.8 kJ/mol. The pressure at sea level is 760 mmHg. Note 1: The P₁ is the pressure at sea level and P₂ is the pressure on Mt. Everest. Note 2: The T₁ temperature is the boiling point of water at sea level which is 100 °C or 373 K. Note 3: The term AHvap is express in kJ/mol. This must be converted to J/mol. a) Using the two component Clausius-Clapeyron equation, determine the boiling point of water on the top of Mt. Everest. InP1/P₂= AHvap/R(1/T2-1/T1) 4

The pressure in a car tire is 28.7 psi at 27 °c. At the end of a trip on a hot day, the pressure has risen to 32.6 psi. What is the temperature of the air in the tire (in Celsius)? The volume of a gas filled balloon is 30.0 L at 40 °C and 1.5 atm pressure. What volume will the balloon have at standard temperature and pressure (STP)? A 5.00 L air sample at a temp of -20 °C has a pressure or 735 mmHg. What will be the new pressure if the temperature is raised to 102 °C and the volume expands to 7.00 L?