Term
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Definition
M vs. m
mols solute/liters solution vs. mols solute/kg solvent |
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Term
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Definition
1) Like dissolves like- two substances with intermolecular forces of about the same type and magnitude
2) Endothermic reactions (H>0)- increase in temperature, increase in solubility
Exothermic reactions (H<0)- incease in temperature, decrease in solubility
3) Pressure (gas-liquid systems)- increasing pressure increases solubilty |
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Term
| Zero Order, First Order, and Second Order reactions |
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Definition
First- ln(Ao/A)=kt
half life t= 0.693/k
Zero- [A]=[A]o-kt
rate=k
Second- rate=k[A]^2
[A]-[A]o^-1=kt |
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Term
| Colligative Properties of Nonelectorlytes |
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Definition
Vapor pressure lowering
Osmotic pressure
Boiling point elevation
Freezing point depression
Depend primarily on concentration of solute particles |
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Term
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Definition
| directly proportional to solute mol fraction |
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Term
| Boiling point elevation/Freezing point lowering |
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Definition
Raise boiling point and lower freezing point
Direct result of vapor pressure lowering |
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Term
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Definition
| water moves from region where its vapor pressure or mole fraction is high to one in which its vapor pressure or mole fraction is lower |
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Term
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Definition
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Term
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Definition
| Solution containing amounts of both weak acid and its conjugate base |
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Term
| What makes an indicator a good indicator for a specific buffer system? |
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Definition
| Point at which it changes color (its end point) is the equivalence point |
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Term
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Definition
| solubility product constant |
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Term
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Definition
randomness factor
Increase temperature- increase entropy
Pure substances always have positive quantities
Aqueous ions may have negative S values
Number of moles of gas increases, so does entropy |
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Term
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Definition
| Ssystem + Ssurroundings = Suniverse >0 |
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Term
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Definition
G<0 spontaneous
G>0 not spontaneous, reverse is
G=0 equilibrium |
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Term
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Definition
G=H-TS
H<0, exothermic reactions tend to be spontaneous
S>0 entropy change is positive, spontaneous if products are less ordered than reactants |
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Term
| Standard Free Energy Change |
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Definition
G<0 spontaneous at standard conditions
G>0 reaction is nonspontaneous at standard conditions
G=0 equilibrium at standard conditions |
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Term
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Definition
| Calculated from heats of formation |
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Term
Effect of
Temperature
Pressure
Concentration
on Reaction spontaneity |
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Definition
Temperature- impossible to change spontaneity with temperature alone
Pressure- G=G0 + RTlnQ
Concentration- ^ |
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Term
| Spontaneity of Redox Reactions |
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Definition
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Term
| Changing concentration and its effect on voltage |
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Definition
Increase concentration of reactant or decrease concentration of produce will increase voltage
and vice versa |
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Term
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Definition
ANODE (marked negative pole of cell)- electrongs are produced by the oxidation half-reaction and pumped into the external circuit
CATHODE- Electrons generated at anode move through the external circuit to the cathode, electrons are consumed |
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Term
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Definition
| Cations move from anode to cathode, anions move to anode |
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Term
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Definition
1) beta particles identical to properties in electrons
2) alpha particles, 42He
3) gamma rays, high energy radiation |
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Term
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Definition
1) Alpha particle emission
2) Beta particle emission
3) Gamma radiation emission
4)Positron emission, same as beta but positive
5) K-electron capture, negative electron in reactants |
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Term
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Definition
| stable nucleus is converted ot once that is radioactive, which in turn decays into stable products |
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Term
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Definition
1) neutron- product nucleus decays by beta emission
2) charged particle |
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Term
| Nuclear fission vs. fusion |
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Definition
| Breaking up heavy nucleus into smaller nuclei utnil mass numbers near maximum vs. combining light nuclei to form a heavier nucleus |
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