Chemistry Exam

Boyles Law

P1V1= P2V2

* inversely proportional

Charles Law

* directly proportional
* temperature must be in Kelvin (Celsius + 273)

Amonton’s Law (Gay-Lussac)

P 1/T 1 = P 2/T 2

* directly proportional
* temperature must be in Kelvin (Celsius + 273)

Combined Gas Law

* directly proportional

Ideal Gas Law

PV = nRT

* P = pressure (ATM)
* V= volume (L)
* n = number of moles
* R= 0.0821 L \* atm / Mol k
* T= temperature (K)


* both direct and inverse

The Kinetic Molecular Theory

Kinetic molecular theory states that gas particles are in constant motion and exhibit perfectly elastic collisions.

● Gas molecules move in straight lines \n ● Gas molecules have no volume \n ● Gas molecules do not attract or repel each other \n ● Gas molecules move at the same speed at a given \n temperature \n ● Gas collision are elastic

Pressure Conversions

1 atm = 760 mm Hg = 760 torr = 101.3 KPa = 14.7 Psi = 101300 Pa

\
* Sea Level Pressure = 1 atm

Solution

solute dissolved in a solvent

Solvation

the process of surrounding solute particles with solvent particles to form a solution

Solute

stuff being dissolved

Solvent / Universal Solvent

\
able to __dissolve__ other substances.

* Water
* capable of dissolving more substances than any other liquid

Miscible

two liquids that are soluble to each other

Solubility

maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure

What affects solubility?

Temperature

* increase in the temperature of the solution increases the solubility of a solid solute.
* the solubility of the gas in a liquid solution decreases with increase in temperature

Pressure

* solubility of gas increases as external pressure increases
* Changes in pressure have essentially no effect on the solubility of solids and liquids.

Polarity

* If the solvent is polar, like water, then a larger dipole moment, indicating greater molecular polarity, will tend to increase the solubility of a substance in it.

Stirring

* allows the solute to dissolve faster.

Molecular size

* Solubility decreases as the molecular size increases.

What are the 4 colligative properties of solutions?

* vapour pressure lowering, boiling point elevation, freezing point depression and osmotic pressure. (the minimum pressure that must be applied to a solution to halt the flow of solvent molecules through a semipermeable membrane)

Consumer (Percent Soln, Percent Sol)

mass of solute/ mass of solution \* 100

vol of solute/ vol soln \* 100

Morality

* the number of moles of solute dissolved in one liter of solution

Acids

any species with an H+ proton

* sour
* little pH (less than 7)
* lithmus paper test turns red/ pink

Bases

any substance with an OH-

* bitter
* slimy
* Big pH (greater than 7)
* lithmus paper turns blue

pH

The pH scale is logarithmic, meaning that an increase or decrease of an integer value changes the concentration by a tenfold

* pH = -log \[H+\]
* pOH= -log \[OH-\]
* pH +pOH = 14

Six Strong Acids

* HBr
* HCl
* HI
* HNO3
* H2SO4
* HClO4

Acid Nomenclature

acids are named using the anion because the cation is always H+

* if anion ends with “ide” then say “hydro” + anion root + “ic” acid
* if anion ends with “ate” then say anion root + “ic” acid
* if anion ends with “ite” then say anion root + “ous” + “acid”

Amphoteric

able to react both as a base and as an acid.

Bronsted/ Lowry Acid

* A Brønsted-Lowry acid is any species that can donate a proton (H+) to another molecule.
* acid is a proton donor
* A Brønsted-Lowry base is any species that can accept a proton from another molecule
* proton acceptor

Arrenhius Acid

is any substance that produces hydrogen ions when dissolved in water.

IMFs

attraction etween molecules

* LDF - when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.
* Dipole- Dipole: all polar molecules
* Hydrogen Bonds: polar molecules with hydrogen bonded with N, O, F

Phase Changes

Autoionization

 a process by which an excited atom becomes ionized and goes to a lower energy state by emitting one of two or more excited electrons that together possess energy exceeding the atom's ionization energy.

What are the 4 ways to decrease solubility?

decrease surface area (larger chunks), decrease \n temperature, decrease pressure (gas), don’t stir or shak

A 2.50 L flask is filled with propone gas, C3H8, at a pressure of 760 torr and at a temperature of -26 C. How many moles of propane gas are contained in the tank?

0.12 mol

A weather balloon is filled with helium that occupies a volume of 52000 L at 101 kPa and at 32 C. After is it is relased, it rises to a location where the pressure is 71.7 kPa and the temperature is -23 C. What is the volume of the balloon at the new location?

6000 L

The air in a dry, sealed 2-L soda bottle has a pressure of 0.998 atm sea level at temperature of 37.0 C. What will be its pressure if its brought to a higher altitude where the temperature is only 25.0 C?

0.959 atm

Raising the temperature of a gas fixed volume container will most likely change the (Amonton’s)

pressure exerted by the gas in the container

When a sample of a gas is kept at constant pressure, the volume and kelvin temperature of the gas are (Charles’)

directly proportional

If the amount and temperature of a gas are kept constant, the pressure and volume of the gas are (Boyle’s)

inversely proptional

A fixed amount of gas is held in a 1.00 L tank of pressure at 3.00 atm. The tank is connected to an empty 3.00 L tank by a tube with a valve. After this valve has been opened and the gas is allowed to flow freely between the two tanks at a constant temperature, what is the final pressure in the system? (volume of the tube is negligible)

0\.75 atm

What is the volume of a gas when the temperature is extrapolated to zero?

the volume would be zero

determine how the volume of a gas (at constant pressure) is related to the absolute temperature

they are directly proportional to each other

what would be the volume of a sample of has at 600 K if its volume at 300 K was 100 liters

200 Liters

In addition to hydrogen, what other atoms are most common in compounds that have hydrogen bonds?

any of these (N, O, F)

Water has unique and unusual properties because of the

hydrogen bonds between polar water molecules

Dipole- dipole forces would most likely to be found in compounds made up of atoms

different electronegativity

Which of the following would indicate the strongest intermolecular forces in a liquid?

high boiling point

The state in which a substance exists at room temperature depends on

strength of the attractive forces between particles

A liquid that has a high viscosity  measure of a fluid's resistance to flow.) would likely have

strong intermolecular forces

What phase(s) of water would be present at 15 C and 200 mm Hg?

liquid

Where would you find boiling water?

at any point along the line separating regions b and c

If the temperature of a sample at 0 C and 25 mm Hg is reduced at constant pressure, what would happen to the sample?

the sample would not change

How could you convert a sample of water at 10 C and 20 mm Hg to vapor without decreasing the temperature?

decrease the pressure to 5 mm Hg so conditions for the sample fall below the solid line