final exam

Chemistry 130 with Yang/zhoa at University of Tennessee - Knoxville

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By: Anonymous
Created: 2010-04-27
Size: 46 flashcards
Views: 1031

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Info about the test (per Dr. Green)

Probably about 5 pts from final lecture material
95 pts from old quizzes about 13-14 pts per quiz (probably 2-4 questions)

Per Dustin

Same format as quizzes
No True and False but know the concepts that were presented in T &F questions

Quiz 1 -Chapter 12

Molarity (M)= moles solute/ liters solution
Molality (m)= moles solute/ kg solvent
Colligative properties- physical properties that depend on the # of particles, not the type of particles
Calculate boiling point elevation and freezing point depression

Molarity (M)

moles solute/ liters solution

Quiz 2- Chapter 13

Know 0 order and 1 st order rate laws (S is always to the -1 exponent!)
Rate = -1/a([A]/t) = -1/c([C]/t), for the reaction aA cC
Integrated rate law (same as what we did in ch 19 but k is )
AM quiz 2 #3, PM quiz 2 #3: Use the balanced equation and the data to answer the following questions

Molality (m)= moles solute/ kg solvent

To go between the two you must know: 1) the density of the solvent to get volume of solvent and 2) the volume of the solute and solvent to get total volume of the solution

Molality (m)

moles solute/ kg solvent

Calculate boiling point elevation and freezing point depression

T f = T f(solution)
T b = T b(solution) ? T b(solvent) = k b x m

T f = T f(solution)

T f(solvent) = -k f x m

Integrated rate law (same as what we did in ch 19 but k is )

Ln([N t ]/[N 0 ]) = -kt

What is the order of fluorine in the rate law equation of this reaction

0 order

What is the overall order of the equation

5 th order

Le Châtelier’s Principle

when any change in concentration, temp, pressure, or volume is imposed on a system at equilibrium, the system responds by attaining a new equilibrium condition that minimizes the impact of the change

Quiz 3- Chapter 14

Equilibrium- condition where the forward reaction and the reverse reaction proceed at the same rate
Don?t worry about the problems with quadratic formula
Equilibrium constant expression- the ratio of equilibrium constants raised to the power equal to the stoichiometric...
Le Ch�telier?s Principle: when any change in concentration, temp, pressure, or volume is imposed on a system at...

Review AM quiz 2 #8, PM quiz 2 #7

Use integrated rate law and half life equation (t 1/2 =0.693/k) to solve

pK w

pK a + pK b

pK a + log [conjugate base]/[weak acid] or pK b +log [conjugate acid]/[weak base]

Quiz 4- Chapter 15

Acid ?Base chemistry is mostly numerical mostly math problems
Only use ICE tables for weak acids and bases, not for strong acids and bases because they completely dissociate in solution
K w = 1 x 10
K w = K a x K b
pK w = pK a + pK b
pH = pK w ? pOH or pK w =pH +pOH
Hydrolysis (could be on final)

Quiz 5- Chapter 16

Henderson- Hasselbalch equation (from ch 15)
K sp expressions- the solubility constant expressions
Relationship of K sp to molar solubility (see AM and PM Quiz 5 #s 8 & 9)
Q ip

K w = 1 x 10

Hydrolysis (could be on final)

See AM and PM quiz 4 # 13

Henderson- Hasselbalch equation (from ch 15)

Only for buffer solutions
pH=pK a + log [conjugate base]/[weak acid] or pK b +log [conjugate acid]/[weak base]

Quiz 6- Chapter 17 &18

Relationships between

K sp expressions- the solubility constant expressions

Only involves the products of the reaction
Will be mostly numerical problems

Relationship of K sp to molar solubility (see AM and PM Quiz 5 #s 8 & 9)

Molar solubility- the molarity of a solute in a saturated aqueous solution

Set up ICE table to find equilibrium values
Convert solubility (g/L) to M and plug M into equilibrium values as s, solve for K sp

Q ip

reaction quotient = the product of the initial concentrations of the products

Q ip > K sp precipitation should occur
Q ip < K sp precipitation cannot occur
Q ip = K sp solution is saturated

Relationships between

Gibbs equation: G = H- TS
Criterion for spontaneous change

Nonspon at all T

G = -RT lnK
Voltaic Cell Components
Balancing Redox Reactions
Quiz 7- Chapters 18-19
Integrated rate law again- use to find and substitute in � life equation
G = -nFE 0 cell
Nernst Equation
Electrolysis

G = -RT lnK

See AM and PM quiz 6 #6

Voltaic Cell Components

Anode- where oxidation occurs, decreases in size, where negative ions flow
Cathode- where reduction occurs, increases in size(plating), where positive ions flow
Salt bridge- completes the circuit
Electrodes- metals (either cathode or anode)

Balancing Redox Reactions

Separate into the � reactions
Balance everything except H and O
Balance oxygen with water
Balance water with H +
Balance charge with e -
Cancel out electrons by multiplication
Combine � reactions
Check that charges are balanced--- STOP HERE IF IN ACIDIC SOLUTION
If in basic solution, add OH - s to both sides and cancel waters

Electrolysis

Example

CrBr 3 + HCl

H 2 O 2H 2 O 4e - + 4H + +O 2

Look at E 0 values for each possible equation, the one with the highest value will occur at the cathode and the one with the lowest value will occur at the anode

-nFE 0 cell

Cathode (reduction)

Cr 3+ Cr 3+ + 3 e - ? Cr

Anode (oxidation)

Br - 2 Br - ? Br 2 + 2e -

About this deck

By: Anonymous
Created: 2010-04-27
Size: 46 flashcards
Views: 1031

About StudyBlue

“I have been getting MUCH better grades on all my tests for school. Flash cards, notes, and quizzes are great on here. Thanks!”
Kathy