V = / 15.0 atmġ) We will manipulate PV = nRT. Since they are both equal (but have different molar masses) you may write: K and 15.0 atm? Assume ideal gas behavior.ġ) Start off by working out how many moles of each gas you have in your mixture.
What is the density of this gas mixture at 500. Problem #34: A mixture of nitrogen and neon gases contains equal moles of each gas and has a total mass of 10.0 g. PV = mRT/M -> n = m/M where m = mass, M = molar mass Problem #33: To identify a diatomic gas (X 2), a researcher carried out the following experiment: She weighed an empty 4.60 L bulb, then filled it with the gas at 1.80 atm and 22.0 ☌ and weighed it again. At what temperature does it have a volume of 7.50 L at 517 mmHg?ġ) The units must match. Problem #32: A gas has a volume of 2.80 L at 1.17 atm and 0 ☌. Since pressure and temperature do not change, there is no volume change. Also, 32 ☏ is the same temperature as zero Celsius and 273 K is the same temp in the Kelvin scale. Solution: It turns out that 722 torr and 0.95 atm are the same pressure. Problem #31: What is the effect of the following change on the volume of 1 mol of an ideal gas? The initial pressure is 722 torr, the final pressure is 0.950 atm, the initial temperature is 32 ☏, and the final temperature is 273 K. Determine the molecular weight of X.ġ) For both gases, P, R, and T are constant. The two containers are at the same pressure and temperature. Problem #30: A 1.00 L container contains 0.20 g of H 2. You would then add x and y to get 349 mmHg.
You could also do this with two Boyle's law calculations and then add the results: The total pressure inside the 6.0 L is found via a Boyle's Law calculation: The hydrogen container expands from 2.5 L (to 6.0 L) and the chlorine container expands from 3.5 L (to 6.0 L). Since moles and temperature remain constant, this problem now reduces to a Boyle's Law problem, involving only pressure and volume. Another way to express this is that the total number of moles of gas does not change. The total number of particles does not change. For every one hydrogen reacting with one chlorine, two HCl are produced. The key factor is the total number of molecules does not change due to the reaction. What is the total pressure inside the two containers at the end of the reaction?
A value (of negligible volume) between the two containers is opened and the gases react irreversibly, following this reaction:Īssume that the reaction goes to completion and the temperature at the end is the same as at the beginning. The two containers are at the same temperature. Problem #29: A 2.5 L container filled with H 2 at 468 mmHg is connected to a 3.5 L container containing Cl 2 at 264 mmHg. (1.5298 x 10¯ 23 cm 3 / atom) (6.022 x 10 23 atom¯ 1 = 9.2124556 cm 3ĥ) Determine the fraction of space occupied by Ar atoms:Ġ.0092124556 / 22.414 = 0.000411 (not a percent, but a decimal amount)Ħ) Determine the percentage of unoccupied space:ĩ9.9589% (I decided to leave it unrounded off.) (1.54 Å) (10¯ 8 cm / Å) = 1.54 x 10¯ 8 cmģ) Using the formula for volume of a sphere, let us determine the volume of one Ar atom:Ĥ) Determine the volume (in liters) occupied by 1.00 mole of the Ar atoms: You might recognize that as molar volume. At STP, that sample occupies this volume: Problem #28: If the argon atom has a radius of 1.54 Å, what percent of an argon gas sample at STP is actually empty space?ġ) Let's assume 1.00 mole of Ar is present. I didn't want to bother looking up (or calculating) R in "L torr/mol K" I converted from torr to atm because I have R in "L atm/mol K" memorized. torr in a 5.01 L container?Ģ) Use PV = nRT to determine the temperature in Kelvin: Problem #27: At what temperature in Celsius will a 1.00 g sample of neon exert a pressure of 500. (c) How big of a container would you need to fit these gases, if you were at 32.0 ☌? (b) What is the partial pressure of each gas? (a) What is the mole fraction of each gas? Problem #26: A container filled with 2.780 mol of N 2, 3.990 mol of O 2, and 13.42 mol of CO 2, has a pressure of 1.252 atm. ChemTeam: Assorted Gas Law Problems 26-50