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CHEM 126 Chapter 13
CHEM 126 Final
| Question | Answer |
|---|---|
| IMAFs on protein | - secondary: form shape - tertiary: overall 3D shape ** determines function - quanternary: arrangement of two or more polypeptide chains in protein |
| IMAFs on DNA | - created by nucleic acids, two chains wrapped around each other in a double helix - polar exterior: PO4 groups interact with ion dipole & h bonds - polar interior: N containing bases, interact by dispersion forces - h bonds: keep chains together |
| colloid | - dispersed (solute-like) substance distributed throughout a dispersing (solvent-like) substances - particles are larger than simple molecules but too small to settle out - EX: G-G (all gases) G-L (foam) L-L (milk) S-L (jelly) |
| Osmotic Pressure (concentration effects) | - increases with number of solute particles - OP = (n solute/ v solution) *RT * n = moles of solute, R = gas constant, T = temp, V = volume of solution) |
| Freezing Point (concentration effects) | - decreases with increasing solute particles -∆T f = ∆Kf*M *m = molality, Kf = freezing point depression constant, ∆Tf = Tf solvent - Tf solution - ∆T > 0 -> decrease in freezing point |
| Boiling Point (concentration effects) | - increases when solute particles increase - boiling point elevation: ∆Tb = Kb * m * Kb = boiling point elevation constant, m = molality, ∆Tb = Tb solution - Tb solvent |
| Vapor Pressure (concentration effects) | - decreases with number of particles of solute (more particles -> lower VP) -P solvent (∆P) = X solvent * P0 solvent * X solvent = 1 - X solute ∆P > 0 -> decrease in VP |
| Parts by Mass (or volume) | - Volume of solute (L)/ volume of solution (L) - composition |
| Mole Fraction | - amount of solute (mol)/ (amount of solute (mol) + amount of solution (mol)) -Vapor-Pressure Determination, Composition |
| Molality | - m - amount of solute (mol)/ mass of solvent (kg) - colligative behavior |
| Molarity | - M - (amount of solute (mol)/volume of solution (L)) - moles of solute that would be dissolved in 1 L of a solution - stoichiometry equations & analysis |
| Henry's Law | - determines gas solubility at given pressures - S gas = K h * P gas * s= solubility (mol/L) Kh = Henry's Law Constant, P = pressure |
| effect of pressure on solubility | - increase pressure -> increase GAS solubility - increase pressure -> decrease does not affect solid of liquid solubility |
| effect of temp on solubility | - increase temp -> increase solid solubility - increase temp -> decrease gas solubility |
| supersaturated | - amount dissolved is more than max dissolved possible - unstable solution & will easily seperate out |
| unsaturated | - amount dissolved is less than max dissolved possible |
| saturated | - max amount of dissolved solid - crystallization rate = dissolving rate |
| sontaneity | energy contribution - entropy contribution * help determine if process occurs spontaneously |
| entropy | distribution of energy over larger number of states |
| ∆H equations | ∆H solution = ∆H solute + ∆ H solvation/hydration (always < 0) ∆H solvation = ∆H solvant + ∆H mixing ∆H solute = -∆H lattice (always > 0) |
| Solubility | - S - max amount that dissolveds in a fixed quantity of a given solvent at a given temp - excess of solute is present |
| different types of solution | L-S (salt water) L-L (gasoline) G-G (natural gas) G-L (soda) G-S (H2 + Pd) S-S (alloys) |
| 2 substances form a solution? | ∆H = exothermic -> unfavorable, will not mix * breaking strong for weak ∆H = endothermic -> favorable & will mix * breaking weak for strong |
Created by:
ccottrel
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