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| What is meant when it is said that a chemical equation is in equilibrium? |
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| The forward rate = the backwards rate |
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| ratio of [products]:[reactants] will reach a constant value |
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| Are stoichiometric coefficients important? |
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| Yes, they are the exponents for the Keq. |
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| Favored towards reactants |
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| expression given for when the equilibrium constant is in terms of concentration |
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| Gives a 'snapshot' of the equation at a given time. Can gain information on which way the reaction should proceed given specific reaction conditions. |
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| Reaction will proceed towards reactants |
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| reaction will proceed towards products |
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| reaction has reached equilibrium! |
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| Kp = Kc(RT)^change in mols of gas |
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| Kc = Kp(RT)^-change in mols of gas |
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| K for a multistep reaction |
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Definition
1. If you know the equilibrium constant for each elementary reaction step, you can calculate the overall K.
EX:
Step 1: A + B -> D K = [D]/[A][B]
Step 2: D -> C K = [C]/[D]
[D] Cancels out, and you are left with: K = [C]/[A][B] |
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K-forward = 1/K-reverse
They are inverses of each other |
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| The free energy change as reactants in their standard states are converted completely to products in their standard states |
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| for reactions in solutions |
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| When does delta G not = 0? |
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| Formula for Delta G of a reaction |
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Definition
| Delta G not+RTln(Q), when R=8.314 |
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| K>1, lnK = positive, Delta G not = negative |
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Definition
| Products are favored at equilibrium |
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| K=1, lnK = 0, Delta G not = 0 |
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Definition
| Products and reactants are favored equally at equilibrium |
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| K<1, lnK = negative, Delta G not = positive |
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Definition
| Reactants are favored at equilibrium |
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Definition
| A system at equilibrium will adjust to an outside stress to re-establish a new equilibrium |
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| What will happen when either a product or reactant is removed? |
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Definition
| The equilibrium will shift towards the deficiency |
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| What will happen when more product or reactant is added? |
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Definition
| The system will shift away from the excess. |
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| What will happen to an endothermic reaction? (LeChatlier) |
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Definition
| An increase in temperature will shift the equilibrium towards the products |
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| What will happen to an exothermic reaction? (LeChatlier) |
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Definition
| An increase in temperature will shift equilibrium towards the reactants. |
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| Increase in pressure / decrease in volume (LeChatlier) |
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Definition
| Shift towards the side with less moles of gas |
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| Decrease in pressure / increase in volume (LeChatlier) |
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| shift towards the side with more moles of gas |
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| Increases the rate of a reaction. DOES NOT affect the equilibrium constant. |
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| What states are not included in ICE tables? |
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| When is a precipitate formed? |
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| When reactants are favored, and the reactant is a solid. |
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| Completely dissociate in water. In water, hydronium is the strongest acid possible. |
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| [Hydronium] > [Hydroxide] |
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| [Hydronium] < [Hydroxide] |
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| [Hydronium] = [Hydroxide] |
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| What forms a conjugate base / acid |
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Definition
A Conjugate base is formed by the reacting acid
A Conjugate acid is formed by the reacting base |
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| Which direction will an acid/base reaction proceed? |
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| Towards whichever side has the weaker acid/base pair |
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| Henderson Hasselbalch Equation |
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| A solution which resists pH changes in the presence of an acid or base |
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Definition
Ability of a buffer to resist changes in pH.
Dependent on:
1. Concentration of buffer: a higher concentration will resist changes more effectively
2. Concentrations of Acid/base pair: a buffer is most effective when pH=pKa. ([acid]=[conjugate base]) |
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