How many moles of gas are now in the flask?ġ) Use PV = nRT with the first set of data to get the volume of the container: The new pressure is 795.0 mm Hg and the temperature is now 26.0 ☌. The flask is now opened and more gas is added to the flask. Problem #14: A sample of gas (1.90 mol) is in a flask at 21.0 ☌ and 697.0 mm Hg. What is the percent composition of the mixture by (a) mass and by (b) volume.ġ) Calculate total moles of gases present:Ĭomment: assume that the volume of the gas mixture is 1.00 L Problem #13: A gas mixture composed of helium and argon has a density of 0.704 g/L at a 737 mmHg and 298 K. V = 24.45388 L (I kept some guard digits)Ĭomment: Titan's atmosphere is five times more dense than Earth's atmosphere. Determine its volume under the conditions of Earth's atmosphere: Assuming ideal behavior, calculate the density of Earth's atmosphere under these conditions.ġ) Let us assume the presence of one mole of gas. Earth's surface temperature is 298 K and its pressre is 1.00 atm. Problem #12: The mean molar mass of the atmosphere at the surface of the Earth is 29.0 g/mol. Determine its volume under the conditions of Titan's atmosphere: Assuming ideal behavior, calculate the density of Titan's atmosphere under these conditions.ġ) Let us assume the presence of one mole of gas. Titan's surface temperature is 95 K and its pressure is 1.6 atm. Problem #11: The mean molar mass of the atmosphere at the surface of Titan, Saturn's largest moon is 28.6 g/mol. ChemTeam: Assorted Gas Law Problems 11-25
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