Properties and KMT
The KMT is a theory that describes this
The behavior of ideal gasses
Dalton's Law of Partial Pressure and the research that accompanied it allowed Dalton to make this critical discovery that reshaped our understanding of the world
The atom
This must always be the unit for Temperature as it is a direct representation of the amount of kinetic energy of the substance
Kelvin
In stoichiometry I always place this on the top of my fraction or conversion factor
The one you are solving for
This property allows gas particles to move through tiny openings in a material
Effusion
According to Charles Law temperature and this variable are directly proportional
Volume
These are the numerical values represented by STP
273 Kelvin and 1 Atmosphere
This is the conversion factor comparing volume and moles
22.4 L = 1 mole
The definition of diffusion is when particles move from areas that are less dense to areas that are more dense.
Explain why this statement is false.
more dense to less dense
According to Boyles Law these two variables are inversely proportional
Pressure and Volume
In the ideal gas law you can solve for temperature with this equation
T=PV/nR
This is the only fraction that will change my starting value if I am converting from Liters of one substance to Liters of another.
The mole ratio
Energy is directly proportional to this property of a gas according to the KMT
What is temperature
In Gay-Lussac's Law we used this common example to describe the direct relationship of its two variables
Tire Pressure
The gas constant represents the standard values of these 4 forms of measurement
Pressure, Volume, Moles, and Temperature
In the reaction:
N2(g) + 3H2(g) → 2NH3(g),
how many liters of hydrogen gas are needed to completely react with 10.0 L of nitrogen gas at constant temperature and pressure?
30 Liters
These are the 5 postulates of the KMT
Gas particles are in constant, random motion.
They move in straight lines until they collide with other particles or the walls of the container.
Gas particles are very small and occupy negligible volume.
The actual volume of the particles is so small compared to the space between them that it can be ignored.
There are no attractive or repulsive forces between gas particles.
Particles neither attract nor repel each other; they move independently of one another.
Collisions between gas particles are perfectly elastic.
When particles collide, no kinetic energy is lost—total kinetic energy is conserved.
The average kinetic energy of gas particles is directly proportional to the temperature in Kelvin.
Higher temperature means higher average kinetic energy of the particles.
This Gas Law is displayed when a student pulls back the plunger of a syringe to draw in air and then seals the tip with a cap. The syringe is then placed in a warm water bath, and the plunger begins to push outward on its own.
Charles Law
A student collects 0.200 moles of a gas in a container at a pressure of 1.20 atm and a temperature of 300 K. Using the Ideal Gas Law, what volume does the gas occupy? (R=.0821)
4.1 L
Avagadro's Law states that all gasses under standard conditions will occupy the same amount of space. Using gas stoichiometry concepts. Explain why 2 Liters of O2 gas might not always produce 2 liters of CO2 gas in a reaction.
If the mole ratio isn't a 1:1