Chemistry Quiz 1 Partial 3 Flashcards
Pass and study for quiz 1 of chemistry partial 3
What does the Law of Dalton’s Partial Pressure of gases say?
The identity of the particle (gas) doesn’t matter, and hence we can add the pressure of different gases to get the total pressure.
Which experiment uses Dalton’s Partial Pressure of gases?
When a reaction is sealed and the resulting gas is led in a tube to water and there the gas is collected along with a bit of water vapor. When we get the pressure a gas exerts in through water collection. When there is more temperature there is more water vapor which means more pressure. Ptotal=Pgas+PH2O
What is the Standard Temperature of pressures (for gases)?
0°C and 1 atmosphere of pressure
Name and explain the Properties of gases, all of them.
•Gases exert pressure( they apply force because they crash into things)
•Gases completely fill a container, they diffuse( they distribute through the container because they move everywhere in chaos and randomly)
•Compressibility, they are compressible( their volume can be reduced, lots of distance between them)
•low density(little mass of large volume, lots of distance again)
•gases are fluids( whatever shape you give them they can flow through it, move around objects and take various shapes because there’s enough space between then and nothing to stop them)
And maybe… They have indefinite shape
Boyle’s Law
PV=k, then P1V1=P2V2. Pressure and volume are inversely proportional. It’s only true when there’s constant pressure.
Charle’s Law
V/T= k, then V1/T1=V2/T2 when there’s constant pressure. The relationship of volume and temperature are linear(directly proportional).
Gay-Lussac’s Law
P/T=k, then P1/T1=P2/T2 when the volume is constant. Pressure and temperature are linear (directly proportional).
Combined gas laws
(PV)/T=k, then (P1V1)/T1=(P2V2)/T2 when only the moles (number of particles is constant). Fusion between boyle’s, charle’s and gay-lussac’s laws. You can get these last laws when you know something is constant.
Gay-Lussac’s law of combining volumes
1 volume of hydrogen per 1 volume of chlorine we get 2 volumes of hydrogen chloride. Remember the ballons. The volumes (ratios) in which the gases react with each other, are always in whole numbers and proportions. Law: For every reaction there’s a whole number for the volumes of reactants with a fixed ratio.
Avogadro’s law
V/n=k. If you double the volume (particles) you have double the volume (particles). When there’s more particles there’s more volume, there’s a proportional relationship between the two of them. Only at constant Temperature and Pressure. In a certain volume, it doesn’t matter the identity of the gas, there will be the same number of particles as long as it is the same volume.
Ideal gas law
PV/nT=k=R R is a gas constant and it’s true for every ideal gas (low pressures and high temperatures), the value changes with different pressure units. Law: PV=nT
Kinetic Molecular Theory
It’s based in that particles are always randomly moving or in motion. This theory only applies to ideal gases and accounts for their properties.
Assumptions/Statements of the Kinetic Molecular Theory
- The particles are much smaller than the distance between them. (They have no volume compared to the space around them, thus we can ignore their volume).
- Collisions between particles of that gas and walls are ellastic collisions (no energy is lost), energy is perfectly transferred and the particles aren’t deformed. In real life the particles would interact(positives and negatives)
- Gases are in rapid, continous random motion. Therefore they posses kinetic energy(KE).
- There are no forces of attraction between gas particles, no repulsions or attractions (Gases do not interact).
- The temperature of the gas depends of the KE of the particles of the gas. Temperature and KE are directly proportional.
Ideal gas
A gas which is in ideal conditions, all gas laws are true for it. It meets the Assumptions/Statements of Kinetic Molecular Theory. At high temperatures and low pressure. They don’t condese.
Real gas
Gas laws aren’t true for it. Doesn’t meet the Assumptions/Statements of Kinetic Molecular Theory. At low temeratures and high pressures. There’s interaction therefore there can be condensation.
