University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2023
Views:

463

Pages:

2
Author:

Ean Mason

Ideal Gas Law Practice Worksheet Solve the following problems using the ideal gas law: 1) How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atmospheres (1.00 atm = 101.3 kPa) and a temperature of 340 K? 2) If I have a 50.0 liter container that holds 45.0 moles of gas at a temperature of 2000 C, what is the pressure inside the container? 3) It is not safe to put aerosol canisters in a campfire, because the pressure inside the canisters gets very high and they can explode. If I have a 1.0 liter canister that holds 2.0 moles of gas, and the campfire temperature is 14000 C, what is the pressure inside the canister? 4) How many moles of gas are in a 30 liter scuba canister if the temperature of the canister is 300 K and the pressure is 20.0 atmospheres? 5) I have a balloon that can hold 10.0 liters of air. If I blow up this balloon with 0.470 moles of helium gas at a pressure of 120 kPa, at what temperature (oC) is the balloon? 6) What is the molar mass of a gas if 10.0 grams of it occupy 2.87 dm3 at a temperature of 25.0oC and 196 kPa? 7) What is the density (in g/L) of Argon gas when the temperature is 35.oC and the pressure is 1.50 atm? Solutions to the Ideal gas law practice worksheet: The ideal gas law states that PV=nRT, where P is the pressure of a gas, V is the volume of the gas, n is the number of moles of gas present, R is the ideal gas constant, and T is the temperature of the gas in Kelvins. 1) 2) 3) 4) 5) 6) 7) 9.9 moles 3.54x103 kPa 2.8x104 kPa 24 moles 340 C 44.0 g/mol (probably CO2) 2.37 g/L