Gas Laws
Name the four laws we have reviewed so far this unit.
Charles'
Boyle's
Gay-Lussac's
Ideal Gas Law
What is Kinetic Molecular Theory?
Theory that explains how gasses behave.
What is a conversion?
Change in form of measurement without changing the actual amount or size.
What is collision theory?
Theory that explains why chemical reactions occur.
How much space does one mole of any substance, at STP, take up?
22.4 L
Inversely related
What is the pressure definition from KMT?
How often and how forceful collisions are.
What value do I use to convert between mass and moles of the same substance?
Molar mass
What are the three postulates of collision theory?
1. Particles must collide
2. Collisions must have sufficient energy
3. Particles must have correct orientation during collision.
What are the four variables of Ideal Gas Law, including units?
Pressure- atm, Pa
Volume- mL, L
n- moles
Temperature- K
List out all of the formulas associated with each law.
P1V1=P2V2 Boyle's
V1/T1=V2/T2 Charles'
P1/T1=P2/T2 Gay-Lussac's
PV=nRT IGL
What is the temperature definition from KMT?
Average kinetic energy of the gas particles.
What two conversions do I need to use if I want to convert the following?
C + O2 ----> CO2
If I have 67g of C, how many moles of CO2 do I have?
Molar mass and mole ratio
Provide an example of something that is not collision theory.
Any physical change.
What are the two Ideal Gas constants? include units!
R = 0.082 L*atm/mol*K
R= 8.31 L* Pa/mol*K
Calculate the unknown.
Throughout the day, my pressure, initially at 6.8 atm, decreases by half. What happens to my initial volume of 2.56 L?
5.12 L
Name a postulate from KMT not regarding pressure or temperature.
1. Gas particles are in constant random motion in straight lines
OR
2. Volume is mostly empty space
OR
3. Gas particles do not stick together; their collisions are elastic
What pressure and temperature must I be at to convert moles to liters of the same substance?
STP
How would a higher temperature affect a chemical reaction?
Higher temperatures mean more collisions because more collisions occur with higher energy. Higher temperatures mean a system has sufficient energy to react.
Calculate the mass of H2S, if I have 78 liters present.
118.7g
Calculate the known.
If I place a 67mL balloon inside my fridge, which reaches a low temperature of 4 degrees Celsius after having it in my 32 degrees Celsius kitchen, what will my final volume be?
0.061 L
How does Kinetic molecular theory connect to Boyle’s Law?
Because KMT tells us that pressure is defined by how often and how forceful collisions are, if we increase volume of a container while maintaining a constant temperature, providing gas particles more room to move freely, the pressure will decrease because frequency of collisions will decrease.
Solve for the following.
N2 + 3H2 ----> 2NH3
If I have 978g of NH3, how many liters of N2 did we start with?
643 L
Why do more reactions occur in the gaseous state?
Since gas particles move more freely, a higher amount of energy increases the speed of gas particles and with the freedom to move around more freely, they collide with one another more often.
How do I convert from Celsius to Kelvin?
Degrees Celsius plus 273