Term
| complex ion formation constant (Kf) |
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Definition
| The equilibrium constant for a complex ion formation. Written like Q, include only aq or g. |
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Term
| Solubility product constant (Ksp) |
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Definition
| The equilibrium established between a solid and aqueous solution (water). The higher the Ksp The more soluble something is. Use Coeefficents as both exponents AND coefficients on s |
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Term
| If you're given one concentration.... |
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Definition
| You can use the Ksp from a table to find the other concentration! |
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Term
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Definition
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Term
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Definition
| A precipitate will not form. |
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Term
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Definition
| The solution is saturated with ions, at equilibrium |
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Term
| An ionic solid is _____ soluble in a solution containing a common ion than it is in water |
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Definition
| An ionic solid is LESS soluble in a solution with a common ion compared to a solution with water. |
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Term
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Definition
| The more soluble something is! |
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Term
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Definition
| When two cations are in solution but only one of them precipitates. The one that requires the lower molarity to precipitate will be the one that does |
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Term
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Definition
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Term
| What can be used to dissolve water insoluble ionic solids? |
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Definition
| Strong acids or complexing agents (like OH- or NH3) |
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Term
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Definition
| A reaction system that moves a system towards equilibrium, increases randomness |
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Term
| Most spontaneous reactions are ____ |
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Definition
| exothermic! but sometimes they're not due to phase change |
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Term
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Definition
| Nature tends to more from low state of probability to high probability. Nature moves towards spontaneity |
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Term
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Definition
| The measure of disorder and randomness |
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Term
| Entropy _____ as temperature increases |
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Definition
| Entropy INCREASES as temperature increases! |
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Term
| Entropy and phase changes |
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Definition
| Entropy increases when going from solid to liquid or liquid to gas |
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Term
| Standard Molar Entropy of Pure Substances |
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Definition
-Only one that is not 0
-Are always positive
-Aqueous ions may have negative molar entropies |
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Term
| Second Law of Thermodynamics |
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Definition
| There is a net increase in entropy during a spontaneous reaction, when the system and its surroundings are in effect. |
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Term
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Definition
| Reaction will be spontaneous |
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Term
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Definition
| Reaction will be non spontaneous |
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Term
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Definition
| The system is at equilibrium |
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Term
| When G(products) < G(reactants) |
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Definition
| The forward reaction is spontaneous |
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Term
| When G(products) > G(reactants) |
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Definition
| The reverse reaction is spontaneous, forward reaction is non spontaneous |
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Term
| When G(products) = G(reactants) |
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Definition
| There is no driving for to make reaction occur |
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Term
| Exothermic reactions tend to be.... |
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Definition
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Term
| Positive Entropy changes tend to be.... |
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Definition
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Term
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Definition
1. use G = H - TS
2. use G(rxn) = G(products) - G(reactants) *Only at 25 Celsius |
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Term
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Definition
- G will always be negative
- The reaction will always be spontaneous |
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Term
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Definition
- G will always be positive
- The reaction will always be non spontaneous |
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Term
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Definition
-At low T, the reaction will be non spontaneous
-At High T, the reaction will be spontaneous |
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Term
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Definition
-At low T, the reaction will be spontaneous
-At high T, the reaction will be non spontaneous |
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Term
| Concentration and Pressure on G |
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Definition
Use the Q equation:
G = G(standard) + RTlnQ
Use Q to solve for effect on G |
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Term
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Definition
Use the K equation:
G = -RTlnK
for the equilibrium constant |
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Term
| Coupling Reactions with G |
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Definition
| Do what we did before by canceling to get desired reaction. Then ADD the G together for the total G |
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Term
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Definition
| a spontaneous redox reaction that can serve as a source of energy |
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Term
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Definition
| Getting "more negative", gaining electrons |
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Term
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Definition
| Getting "more positive", losing electrons |
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Term
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Definition
| Where reduction occurs, so they accept the electrons |
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Term
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Definition
| Where oxidation occurs, so they lose electrons and gain "+ ions" |
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Term
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Definition
| Something that allows the positive ions to flow from the anode to the cathode. |
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Term
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Definition
| When all ions and molecules in a voltaic cell are at a concentration of 1 and all gases are at 1 atm |
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Term
| Standard Voltage Equation |
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Definition
| E(standard) = E(red) + E(ox) |
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Term
| Strength of oxidizing and reducing agents |
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Definition
| The more negative the E(red), the strong the reducing agent it is |
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Term
| When E(cell) is positive.... |
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Definition
| The reaction is spontaneous |
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Term
| When E(cell) is negative... |
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Definition
| The reaction is non spontaneous |
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Term
| E(cell) in a voltaic cell... |
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Definition
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Term
| Relationship with G, E, and K |
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Definition
Use equation G = -nFE
n = the number of moles of electrons transferred
F = farradays constant
E = standard electrical energy |
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