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

744 mmhg to atm