Study better. Learn faster. Get the grade you want.
Discover why millions of students use us to learn better.

Sign up now and start studying these cards for FREE

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 are the units for the rate constant

M -4 S -1

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 Châtelier?s Principle: when any change in concentration, temp, pressure, or volume is imposed on a system at...

What are the units for the rate constant M

- 4 S
- 1

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

K w

K a x K b

pK w

pK a + pK b

pH

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

14

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

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

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

2 4 He

- 2
- 4

Beta

1 0 e

1 0 e

1

Electron Capture

- 1 0 e
- 1

Electrolysis

Example

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

?G

-nFE 0 cell

Cathode (reduction)

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

Anode (oxidation)

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

About this deck

Author: Anonymous

Created: 2010-04-27

Updated: 2011-07-20

Size: 46 flashcards

Views: 1091

Created: 2010-04-27

Updated: 2011-07-20

Size: 46 flashcards

Views: 1091

Simply amazing. The flashcards are smooth, there are
many different types of
studying tools, and there is
a great search engine. I praise
you on the awesomeness.
- Dennis

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

I was destroying whole rain forests with my flashcard production, but YOU, StudyBlue, have saved the ozone layer. The earth thanks you.
- Lindsey

This is the greatest app on my phone!! Thanks so much for making it easier to study. This has helped me a lot!
- Tyson

StudyBlue is not sponsored or endorsed by any college, university, or instructor.

© 2014 StudyBlue Inc. All rights reserved.

© 2014 StudyBlue Inc. All rights reserved.