Chem Test 3

Front 1

What are the S.I. Units of Pressure?

Back 1

1 atm=760 mm Hg=14.7 psi=101.325 Pascals

Front 2

What is Boyle's Law?

Back 2

As volume increase, pressure decreases at constant K (temperature)

P1V1=P2V2

Front 3

What is Charles' Law?

Back 3

As volume increases, temperature increases

Volume of gas at a constant pressure is directly proportional to it's Kelvin Temperature.

V1/T1=V2/T2

Front 4

What is Gay-Lussac's Law?

Back 4

As pressure increases, temperature increases.

Pressure is directly proportional to it's Kelvin Temperature

P1/T1=P2/T2

Front 5

What is the Combined Gas Law?

Back 5

As pressure/volume increases, temperature decreases

The product of pressure and volume is inversely proportional to it's temperature at a fixed amount of gas.

P1V1/T1=P2V2/T2

Front 6

What is Avogardo's Law?

Back 6

As volume increases, moles increase.

Equal volumes of gas at the same temperature and pressure contain equal numbers of molecules.

V1/N1=V2/N2

Front 7

What are the SPT values?

Back 7

Standard Temp= 0C (273K)
Standard Pressure= 1 atm (760 mm Hg)
Standard Molar Volume= the volume of 1 mole of gas at STP = 22.4L

Front 8

What is the Ideal Gas Law?

Back 8

A general expression relating pressure, volume, temperature, and moles for an ideal gas.

PV=nRT

Front 9

What is the universal gas constant?

Back 9

R=0.0821 L(atm)/ or 62.4 L (mm Hg)/
mol (K) mol (K)

Front 10

What is Dalton's Law of Partial Pressure?

Back 10

P(total)=P(gas 1) + P(gas 2)........

Front 11

Name the Intermolecular forces

Back 11

London Dispersion, Dipole-Dipole, Hydrogen Bonding

Front 12

What forms a Hydrogen Bond?

Back 12

Hydrogen bonding occurs when a hydrogen atom bonded to O, N, or F is elctrostatically attracted to an O,N, or F in another molecule. Always occurs with OH

Front 13

What is vapor pressure?

Back 13

Pressure exerted by gas molecules in equilbrium with the liquid phase.

Front 14

Describe Crystalline and amorphous solids

Back 14

Crystalline solids have a regular arrangement of particles, atoms, molecules, and ions with a repeating structure.

Amorphous solids have no regular arrangement.

Front 15

Describe Sublimation and Deposition

Back 15

Sublimation is changing from solid to gas without liquid phase.

Deposition is changing from gas to solid without liquid phase.

Front 16

Define a solution and a colloid

Back 16

A solution is a homogenous mixture that contains small particales.

A colloid is a homogenous mixture with larger particles

Front 17

Describe Solute and Solvent

Back 17

Solute is what's being dissolved

Solvent is what's doing the dissolving

Front 18

Define Solubility

Back 18

The amount of solute that dissolves in a given amount of solvent at a specific temperature. Low solubility = insoluble
High solubility= soluble

Like dissolves like

Front 19

What is the weight/volume concentration formula?

Back 19

w/v% = mass of solution (g) / x 100%
volume of solution (mL)

Front 20

What is the ppm formula?

Back 20

Mass of solute (g) / x 10^6
Mass of solvent (g)

Front 21

Define Dilution

Back 21

Dilution is the addition of solvent to decrease the concentration of solute. The solution volume changes, but the amount of solute is constant.

M1V1=M2V2

Front 22

Describe the Colligative properties of solutions

Back 22

Pure Solvent Soln
Vapor Pressure higher lower
Boiling Point lower higher
Freezing Point higher lower
Osmosis move to equalize concentration

Front 23

What is the Freezing Point Depression formula?

Back 23

Change in Temp = 1.86 C / x mol of particles
mol

Front 24

Define Osmosis

Back 24

The passage of water and small molecules across a semipermeable membrane from a solution of low solute concentration to a solution of higher solute concentration

Front 25

What are isotonic, hyptonic, and hypertonic solutions?

Back 25

Isotonic solutions have the same osmotic pressure.

Hyptonic solutions have lower osmotic pressure than body fluids.

Hypertonic solutions have higher osmotic pressure than body fluids.

Front 26

What happens when molecules react and what energy is required?

Back 26

Bonds are broken in the reactants and new bonds are formed in the products

Bond breaking requires an input of energy and bond formation releases energy.

Front 27

What is the heat of reaction (enthalpy) ?

Back 27

The energy absorbed or released in a reaction.

Front 28

Define exothermic and endothermic reactions.

Back 28

Endothermic reactions are when energy is absorbed from it's surroundings. When delta H is negative.

Exothermic reactions are when energy is released to it's surroundings. When delta H is positive.

Front 29

Define Bond Dissociation energy.

Back 29

The amount of energy required to break a bond and to seperate the atom into isolated gaseous molecules.

Front 30

Define spontaneous and non-spontaneous reactions.

Back 30

Spontaenous reactions are reactions that once started, proceed on their own without external influence.

Non-spontaneous reactions are reactions that require constant external influences

Front 31

Define Entropy

Back 31

The amount of disorder in a system.

Front 32

What is free energy and what is the formula?

Back 32

Free energy is the criteria for a spontaneous reaction.

G=H−TS

Temperature in Kelvin. Negative values mean spontaneous reactions and positive values mean non-spontaneous reactions.

Front 33

What affects the rates of chemical reactions?

Back 33

-Molecular collisions
-Activation energy
-Nature of the reactants
-Concentration of the reactants
-Temperature
-Presence of a catalyst

Front 34

Define a catalyst

Back 34

A substance that speeds up the rate of reaction, but is itself unchanged.

Front 35

What is equilibrium?

Back 35

A state in which the forward and reverse reaction rates are the same.

Front 36

What is the formula for equilibrium?

Back 36

K = [products] /
[reactants]

The coefficients become the exponents.

Front 37

What side does an equilibrium favor?

Back 37

When K is much greater than 1, the numerator is larger, the equilibrium favors the products and lies to the left.

When K is much less than 1, the denominator is larger, the equilibrium favors the reactants and lies to the right.

When K is around 1, both reactants and products are present

Front 38

What is Le Chatelier's Principle?

Back 38

When stress is applied to a system in equilibrium, the system shifts to relieve the stress. Stress equals any change in pressure, temperature, concentration, and/or volume