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CHM 129 > Exam 2 > Flashcards

Exam 2 Flashcards

Lectures 17-26

1
Q

Osmosis

A

selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentration one
* solvent flows from more dilute solution to a more concentrated one

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2
Q

Osmotic pressure

A

pressure required to stop osmosis

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3
Q

Hypotonic solution

A

has a lower concentration of particles than the cell

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4
Q

What happens if a cell is placed in a hypotonic solution

A

water (solvent) rushes into cell, cell swells, and bursts

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5
Q

Hypertonic solution

A

has a higher concentration of particles than the cell

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6
Q

What happens if a cell is placed in a hypertonic solution

A

water moves out of the cell, causing it to shrink

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7
Q

Balancing equations (4 points)

A
  • if only C, H, O in equation, balance it in that order
  • balance a free element at the end
  • balance a metal before a nonmetal
  • don’t seperate polyatomic ions
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8
Q

Combustion

A

reactant: oxygen
product: CO2 and H2O

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9
Q

rate

A

how much a quantity changes in a given time

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10
Q

thermodynamics

A

whether free energy was released or absorbed

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11
Q

collision theory

A

collision frequency
collision energy
collision orientation

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12
Q

What are the 4 factors that affect rate?

A
  1. concentration of reaction
    * direct
  2. temperature
    * direct
  3. physical state
    * 2 liquids = more collisions
    * 1 solid 1 liquid = less
  4. catalyst
    * not consumed
    * only small amount needed
    orient molecules so correct orientation is greater
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13
Q

For each __ rise in temp, the rate of reaction __

A

10 degrees celcius
doubles

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14
Q

rate expression

A

gives relationship between the different rates of change of reactants and products of the same reaction
* reactions are negative
* products are positive

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15
Q

differential rate law

A

relationship between rxn rate and reacatant concentration

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16
Q

Which factor affects k?

A

temperature

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17
Q

Which factor does not change k?

A

concentration

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18
Q

How do you find order of the reaction?

A

add the exponents of the reactants

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19
Q

Sign for rate of appearance and disappearance

A

appearance=+
disappearance=-

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20
Q

Half-life

A

time it takes for half the substance to disappear

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21
Q

relationship between order for half life and concentration

A

0 - direct
1st - no relationship
2nd - inverse

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22
Q

zero order half life gets longer or shorter, why

A

half life gets shorter with time
rate is constant, so it takes shorter time to make substance disappear

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23
Q

For first order half life, which factors depend on concentration and which ones don’t

A

depend on concentration: rate *rate=k[A]
does not depend on concentration: k and half-life

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24
Q

Second order half-life gets longer or shorter, why

A

half-life is getting longer with time because it is dependent on collision, and lower concentration means less collusions

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25
Q

activation energy

A

minimum amount of energy to START a reaction * lowest activation energy is most stable and fastest

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26
Q

transition state

A

when molecules collide effectivelt, they form an activated complex
* partially broken and partially formed bonds
* unstable
* transitional species: partly between reactant and product

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27
Q

How do you find the overall order of the reaction?

A

add the exponents of the reactants

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28
Q

remember

A
  • check if the equation is balanced
  • don’t forget k in rate
  • for elementary reactions (NOT overall reaction), the order can be determined from the coefficients
  • if it says “second decay”, you have to do it twice
  • include units for k
  • some equations line up with y=mx+b
  • make R into kJ if needed
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29
Q

sig fig rule with logs

A

sig figs in answer after decimal point is the same number of sig figs in log

ex. log 4.000 (4 s.f.) = 0.6021(4 s.f. to right of the decimal point)

30
Q

integrated rate law

A

used to determine how long a reaction takes or how much reactant or product is present at a given time

31
Q

key words to know to use the integrated rate law

A

“How long”

32
Q

frequency factor

A

of collisions with correct orientation to react

33
Q

how does temperature affect half life of radioactive decay vs chemical reactions

A

doesn’t affect half life of radioactive decay
affects half life of chemical reactions

34
Q

catalyst

A

consumed then produced

35
Q

intermmediate

A

produced then consumed

36
Q

unimolecular

A

reactant is 1 molecule

37
Q

bimolecular

A

reactant is 2 molecules

38
Q

termolecular

A

reactant is 3 molecules

39
Q

Which molecules are in the rate law?

A

molecules that are in the overall equation

40
Q

3 conditions to validate a mechanism

A
  1. sum of elementary reactions must equal overall balanced equation
  2. rate law for slow step can’t have any intermmediates (if slow step is first, it will never have intermmediates in the rate law b/c intermmediates are produced then consumed (products aren’t included in the rate law; however, if the slow step is not the first step, it could have intermmediates)
  3. slow step must have same rate law from experimental data
41
Q

When do you vs do not subsitute?

A
  • substitue when there is a fast initial rate followed by slow step w/ intermmediates
  • don’t substitute when there is a slow initial step w/ intermmediates
42
Q

2 conditions to check when writing the overall rate law

A
  1. if the molecules are included in the overall equation, include it in the rate law
  2. is the slow step first w/ intermmediates? if not first step w/ intermmediate, need to substitute
43
Q

intermmediates

A

not reactants or products

44
Q

catalysts

A
  • increase rate of forward and reverse reactions
  • a catalyzed rxn yields the product more quickly but it’s the same amount of product
45
Q

enzymes

A
  • biological catalyst
  • most are proteins
    *bind substrate (reactants) in active site and orients it for rxn
    *highly specific
    (1 enzyme: 1 reaction)
  • doesn’t alter amount of energy consumed
46
Q

How do enzymes attract and hold substrate?

A

weak non-covalent interactions ex. hydrogen bonding, hydrophobic interactions, ionic interactions

47
Q

lock and key model

A
  • enzyme = lock
  • substrate = key
48
Q

Why is the lock and key model not the best model

A

the substrate has to fit perfectly for the enzyme to work
* if no strong interactions, enzyme and substrate complex will fall apart so no products will be produced

49
Q

induced fit enzyme model

A
  • active site is flexible pocket whose shape changes to accomodate substrate molecule
  • after, product doesn’t fit in active site and is released
50
Q

binding energy

A

free energy released in forming multiple weak bonds + interactions between an enzyme and its substrate

51
Q

How do enzymes lower activation energy?

A

*puts molecules in close proximity to react and collide
* analogy: wingman

52
Q

saturated

A

so much substrate that the rate is limited by enzyme availability; all active sites are occupied

53
Q

competitive inhibitor

A

competes w/ substrate for active site on enzyme and is a similar structure as the enzyme
* solution: increases concentration of substrate because this increases chance

54
Q

noncompetitive inhibitor

A

bind to location other than active site, changing shape of enzyme; substrate can’t bind to enzyme anymore
* solution: move inhibitor

55
Q

irreversible inhibitor

A

inhibitors covalently change active site permanently
* solution: wait for more enzyme

56
Q

what stays the same in competitive inhibition

A

Vmax

57
Q

what stays the same in non-competitive inhibition

A

Km

58
Q

Lineweaver-Burk plot
* x-axis (units)
* y-axis (units)
* x-intercept
* y-intercept

A

x-axis: 1/[S] (m/M)
y-axis: 1/V (1/micro moles)
x-intercept: -1/Km
y-intercept: 1/Vmax

59
Q

Michaelis-Menten plot
* x-axis (units)
* y-axis (units)
* x-intercept
* y-intercept

A
  • x-axis: [S] (mM)
  • y-axis: V (micro moles)
  • x-intercept: Km
  • y-intercept Vmax
60
Q

emission

A

particles goes on right side of arrow
* emission means release
* look for “decay”, “production”, “formation”

61
Q

capture

A

particle goes on left side of arrow
* look for “absorption”, “bombardment”

62
Q

gamma decay

A

no particles emitted

63
Q

What order is radioactive decay?

A

1st order

64
Q

how does length half-life length affect temperature

A

shorter half-life means more nuclei decay every second which means hotter

65
Q

does temperature affect rate of change in radioactive decay

A

no

66
Q

How to find grams of excess reactant?

A

substract moles of product, do moles to moles of excess reactant and convert that into grams of the excess reactant

67
Q

from a graph, how do you know which step is the rate-determining step and how do you know the intermmediates

A

*the one with the highest activation energy
* the bumps are the steps, so look at which bumps the intermmediate is in between

68
Q

what is the slope for differential and integrated rate law

A
69
Q

order and half life

A
  • 0 = half life decreases over time
  • 1st = half life remains constant
  • 2nd = half life increases over time
70
Q

how to write the rate law when there are 3 reactants

A

hold the other 2 reactants constant

CHM 129 (4 decks)

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