Key Concepts
What is the gaseous state of any substance that normally exists as a liquid or solid?
Vapor
Boyle's Law relates pressure and volume at constant ______.
Temperature
What is the equation for the Ideal Gas Law?
PV=nRT
At STP, what is the volume that 1 mole of an ideal gas occupies?
22.4 L
Ideal gases assume no _____ between gas particles?
Intermolecular forces
What is the units commonly used to measure gas pressure in chemistry?
atmosphere (atm)
Charles's Law states that as a temperature increases, volume ______.
Increases
What is the term R in the ideal gas equation called?
gas constant
How many liters of O2 are produced from 2.0 moles at STP?
44.8 L
Real gases deviate most from ideal behavior under which two conditions?
Low temperature and high pressure
What is the law that states that the total pressure of a mixture of gases is the sum of the partial pressures?
Dalton's Law of Partial Pressures
Gay-Lussac's Law deals with the relationship between pressure and ______.
Temperature
What is the value of R when using atm and liters?
0.0821 L·atm/mol·K
What volume of CO2 is produced from 2.0 g of C at STP?
1.87 L
Out of which of the following, which gas would behave most ideally at room temperature, He, H2O, or NH3?
He
What are the 4 variables used to describe a gas?
Pressure, Volume, Temperature, and moles
A gas at 2.0 atm and 3.0 L is compressed to 1.0 L. What is the new pressure?
6.0 atm
Calculate the pressure of 1.0 mole of gas in a 2.0 L container at 300 K.
12.3 atm
A reaction produces 5.6 L of H2 at STP. How many moles is that?
0.25 mol
Which gas law includes correction factors for intermolecular forces and volume?
Van der Waals equation
What temperature scale must be used in gas law calculations?
Kelvin
A gas at 300K occupies 2.0 L. What volume will it occupy at 600 K and constant pressure?
4.0 L
If 4.0 g of He is in a 10.0 L container at 273 K, what is the pressure?
2.24 atm
N2 + 3H2 → 2NH3
According to the equation above, how many grams of H2 are needed to produce 22.4 L of NH3 at STP?
3.0 g
Why do gases behave ideally at high temperature?
Particles have enough kinetic energy to overcome intermolecular forces