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What is a closed system?
energy can change, mass cannot
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Describe Extensive Properties
A property that changes with the amount of material
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Describe Intensive Properties
A property that does not change with the amount of material
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State Functions are...
pathway independent
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Path functions are
pathway dependent
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Conduction
direct contact, molecules are transferring energy
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Convection
through fluid movement
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Radiation
transfer of energy through electromagnetic waves
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Relate pressure, volume and work
W=PΔV
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How to convert Celsius to Fahrenheit
F =  C + 32
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First Law of Thermodynamics
Conservation of energy. Energy is neither created nor destroyed, but in interconverted
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Zeroth Law of Thermodynamics
When two systems are at thermal equilibrium with a third, they are also at equilibrium with each other
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Second Law of Thermodynamics
- Heat cannot be changed completely into work in a cyclical process
- Entropy will always increase
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Third Law of Thermodynamics
Assigns zero entropy to a pure substance at absolute zero and in internal equilibrium
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Enthalpy
Give equation, describe what positive and negative are
- the change in heat
- ΔH = ΔU + PΔV
- +ΔH = endothermic
- -ΔH = exothermic
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Breaking bonds (releases/uses) energy?
Uses
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Forming bonds (releases/uses) energy?
releases
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Gibbs free energy:
give the equation
What is spontaneous?
- ΔG = ΔH-TΔS
- -ΔG = spontaneous
- +ΔG = nonspontaneous
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Colloids
- solid + liquid or
- gas + liquid
- can be separated by a semi-permeable membrane
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lyophilic
solutes attracted to solvent
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lyophobic
solutes not attracted to solvent
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molality
m =
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mole fraction
weird X =
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parts per million
ppm = X 10 6
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1 mol of gas = how many liters?
22.4 L
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How many torr is 1 atm?
760 torr
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When forming a solution, ΔS (entropy) always...?
increases
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How do you find the ΔH of the formation of a solution?
It is equal to the ΔH for all steps
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Negative heats of solution form ____ (stronger/weaker) bonds and _____ (higher/lower) vapor pressure
stronger, lower
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Lewis definition of Acid/base
- Acid = accepts pair of electrons
- Base = donates pair of electrons
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Bronsted-Lowry definition of acid/base
- Acid = donates proton
- Base = accepts proton
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Arrhenius definition of Acid/Base
- Acid = anything that produces H+ ions in aqueous solution
- Base = anything that produces OH- ions in solution
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With increasing polarity, acidity _______?
increased polarity = decreased acidity
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Give the expression for Ka
K a =
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What is important about the 1/2 equivalence point?
there is 50% HA(acid) and 50% A- (conjugate base)
and pH=pKa
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What is Raoult's Law?
P v = X aP a
- Pv = vapor pessure of a solution
- Xa = mole fraction
- Pa = vapor pressure of pure liquid a
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Henry's Law demonstrates what?
that the solubility of the gas is proportional to its vapor partial pressure
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Head capacity = ?
C = q/ΔT
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Specific heat of water is?
1 cal/g°C
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What is critical temperature?
The temp. at which a substance cannot be liquefied no matter how much Pressure is added
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Critical Point
beyond this point, an increase in temperature and/or pressure cause the substance to have both gas and liquid properties
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osmotic pressure = ?
- Π = iMRT
- Π (pi) = osmotic pressure
- i = van't Hoff factor
- M= molarity
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Van't Hoff Factor
The number of particles that a given molecule will separate into if put into an aqueous solution
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Change in boiling temperature = ?
ΔT = k bmi
- Kb = specific constant for substance being boiled
- m=molality
- i= van't hoff factor
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With increased bond strength, acidity is _____?
decreased
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A larger pKa means a (stronger/weaker) acid?
weaker
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what is K of water at 25°C?
Kw = 10-14
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What is the Henderson-Hasselbalch equation?
pH = pK a+ log
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What happens at the cathode?
reduction
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What happens at the anode?
oxidation
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The substance being oxidized is the...?
Reducing agent
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The substance being reduced is the...?
Oxidizing agent
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What is the oxidation state of oxygen?
-2
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What is the oxidation state of Fluorine?
-1
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What is the oxidation state of Hydrogen?
+1
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A positive cell potential indicates a _______ (+/-) ΔG and a _________ (spontaneous/non-spontaneous) reaction
negative ΔG, spontaneous
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electrolytic cells have ________ (+/-) cell potential
negative
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Galvanic/voltaic cells have a _______ (+/-) cell potential
positive
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