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Chem Exam 1
| Question | Answer |
|---|---|
| If Q is less than K in an equilibrium reaction then | it must keep going to catch up (so reaction goes in forward/right direction) |
| volatility | tendency of a liquid to vaporize |
| Clausius-Clapeyron is for | enthalpy of vaporization |
| 1atm=?torr | 760 torr |
| moles formula | mass (g) / molar mass (g/mol) |
| molarity formula | moles of solute / L of solution |
| is molarity volume or mass based? | volume based, think mol-air, volume, so temperature affects it |
| dilution formula | M1V1=M2V2 both should be in either mL or L |
| is molality volume or mass based? | mass based, so temperature doesn't affect it |
| molality formula | moles of solute / mass (kg) of solvent |
| boiling point elevation steps | convert grams->moles, find molality, input into formula |
| freezing point depression | convert grams->moles, find molality, input into formula |
| boiling and freezin gpoint both use | ∆T=imK, but when boiling, adding/elevation, freezing is a depression/subtraction |
| intermolecular forces describe and examples: | attractive forces between molecules + atoms, london dispersion, dipole-dipole, hydrogen bonding, ionic bond |
| dipole-dipole | non-symmetrical, but polar |
| london dispersion force | single element, or symetrical nonpolar |
| hydrogen bonding | H DIRECTLY bonded to a F, O, or N |
| ionic bond | metal + nonmetal, opposites attract, one loses one gains electrons |
| what changes k in equilibrium? | only temperature, because it affects balance between reactants and products |
| temperature effect on exothermic reactions | exo- temp up, lower k (produces heat, heat is product) |
| temperature effect on endothermic reactions | endo- temp down, lower k (absorbs heat, heat is reactant) |
| Kc if K is greater or less than 1 | K>1, products favored (more products than reactants, democrat, majority of good people), K<1 reactants favored (more reactants than products, conservatives are reactive and make up less of population) |
| endothermic/exothermic reactions heat trick | ADD heat, reaction shifts away from that side. REMOVE heat, reaction shifts towards that side |
| what affects reaction rates? | temp, concentration, surface area, nature of reactants, catalyst |
| dipole-dipole is permanent polarity due to attractive forces | |
| london dispersion forces are temporary polarity due to unequal electron distribution | |
| hydrogen bonding is a strong dipole-dipole | |
| surface tension has a higher or lower potential energy? | higher, less neighbors so they're less stable than those in interior |
| intermolecular forces and temp on surface tension | stronger intermolecular forces, higher surface tension. raised temp makes molecules shake, weakening intermolecular forces, reducing surface tension |
Created by:
AKDakd