Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

flash > diploma studying > Flashcards

diploma studying Flashcards

1
Q

thermochemistry

what is Q=mcΔt mean, and what do the individual elements represent?

A

-used to calculate heat transferred in a process with no phase change
- Q = quantity of heat transferred into the system
m = mass (g)
c = specific heat capacity
Δt = temperature change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

thermochemistry

what is the origin of chemical bond energy?

A

(majority of biosphere) is derived from solar energy
- energy required to break bonds
- energy released when bonds break

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

thermochemistry

what is enthalpy?

A
  • change in potential energy between reactants and products
  • represented by ΔH (or ΔrH)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

thermochemistry

what is molar enthalpy?

A
  • enthalpy per mole of specified substance
  • represented by ΔH, or ΔHm
  • units in kJ/mol
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

thermochemistry

how do you find amount of energy released or absorbed in reaction (equation)

A

ΔH = nΔrH
ΔH = enthalpy change
n = #of moles of specific substance
ΔrH = molar enthalpy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

thermochemistry

how do you find standard enthalpies of formation

A

ΔrHº = Σ(nΔfHº)products - Σ(nΔfHº) reactants
Σ = “sum of”

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

thermochemistry

what is calorimetry, the equation, and individual representations?

A
  • energy lost/gained by system observed by (equal to) changes in water temperature
    ΔH = -Q = -mcΔt
    m = mass of water
    c= specific heat capacity of water
    =Δt is change in water temperature
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

thermochemistry

what is a bomb calorimeter

A
  • different material other than polystyrene used
  • heat absorbed must be accounted for
    formula: nΔrH = CΔt
    C=constant, heat capacity of calorimeter
    no need for mass
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

thermochemistry

states of water in organic reactions

A
  • photosynthesis and cellular respiration both produce/consume LIQUID water (closed systems)
  • in open systems (e.g. combustion), GASEOUS water will be produced
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

thermochemistry

ΔH, endothermic and exothermic

A

ΔH positive = endothermic
ΔH negative = exothermic
photosynthesis is endothermic, while combustion and cellular respiration is exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

thermochemistry

what is activation energy

A
  • Ea, minimum collision energy to produce a successful reaction
  • (KMT) = need sufficient speed and orientation to occur through collisions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

thermochemistry

breaking/forming bonds in relation to endothermic and exothermic reactions

A
  • exothermic = products contain less potential energy than reactants
    -endothermic = products contain more potential energy than reactants, require more kinetic energy to create activated complex (extra energy stored in bonds of products)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

thermochemistry

catalysts and their effects

A
  • cause rate of reactions to increase by providing an alternate pathway (less energy needed)
    does NOT affect value of ΔH, change reactants/products, or get consumed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

electrochemical changes

what is oxidation and reductions

A

oxidation: loss of electrons, substance is oxidized
reduction: gain of electrons, substance is reduced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

electrochemical changes

what is a redox reaction

A

two processes do not occur in isolation
net reaction, “reduction-oxidation reaction”

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

electrochemical changes

what are oxidizing and reducing agents?

A

oxidizing agent: GAINS electrons (reduced), causes another substance to get oxidized
reducing agent: LOSES electrons (oxidized), causes another substance to get reduced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

electrochemical changes

what is disproportionation?

A
  • redoc reaction where the SAME substance functions as both the RA and the OA
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

electrochemical changes

what is an oxidation #, and relation to oxidation and reductions

A
  • positive or negative number, allows you to determine the movement of electrons in a reaction
    increase: substance is being oxidized
    decrease: substance is being reduced
    H is ALWAYS +-1, O is always -2
    *easiest way to determine if a reaction is a redox rxn or not
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

electrochemical changes

what is the rule of spontaneity?

A

if the OA is above the RA on a table of half-reactions, the reaction is spontaneous. If not, it is non spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

electrochemical changes

balance out redox reactions
(from half reactions)

A
  1. write half reactions
  2. multiply coefficients to balance electrons
  3. add half reactions to obtain balanced net reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

electrochemical changes

balance out redox reactions (creating own half reactions)

A
  1. balance all molecules except O and H
  2. Add H2O to balance O
  3. Add H to balanced H
  4. Balance electrons
  5. write out half reactions
  6. multiply one half reactions to match electrons in other half reaction
  7. add together to obtain net reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

electrochemical changes

balance out redox reactions (from OA and RA)

A
  1. identify OA and RA
  2. balance electrons
  3. balance primary atom
  4. balance oxygen with H2O
  5. balance H
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

electrochemical changes

what is a voltaic cell

A

-spontaneously reaction to produce electricity
E net: positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

electrochemical changes

what is an electrolytic cell

A
  • uses electricity to cause non spontaneous reaction (electrical>chemical energy)
    E net: negative
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

electrochemical changes

what is the electrode

A

solid in half cell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

electrochemical changes

what is the anode

A

electrode where oxidation occurs (SRA reacts)
voltaic: negative charge
electrolytic: positive charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

electrochemical changes

what is the cathode

A

where reduction occurs (SOA reacts)
voltaic: positive charge
electrolytic: negative charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

electrochemical changes

what is an anion and cation

A

anion: negative ion, moves to anode
cation: positive ion, moves to cathode

29
Q

electrochemical changes

what is a salt bridge/porous cup

A
  • barrier which keeps solutions of voltaic cells apart, but allows ion flow
30
Q

electrochemical changes

what is an electrolyte

A
  • substance that conducts electricity when dissolved in water
  • solutions in both cells
31
Q

electrochemical changes

what is a power supply

A

electronic device that replaces a battery
- drives electrolysis reactions

32
Q

electrochemical changes

what is the external circuit

A

wires (and voltmeter) that are used to connect anode to cathode
electron flow from the anode to the cathode

33
Q

electrochemical changes

what is the line notation for cells

A

anode|anode electrolyte||cathode electrolyte|cathode

34
Q

electrochemical changes

what is the chloride anomaly

A

when H2O ( in presence of CL) is both the SRA and SOA, chloride will become the SRA (anode rxn)

35
Q

electrochemical changes

what are standard reduction potentials

A

Erº, measured to the standard hydrogen half cell (Erº=0.00V)

36
Q

electrochemical changes

how to calculate standard cell potential

A

Eºnet = Erºcathode - Erºanode
positive: spontaneous
negative: non spontaneous

37
Q

organic chemistry

what are organic compounds, and exceptions?

A
  • molecular compounds of carbon
    exceptions: oxides, and ionic compound containing carbon
38
Q

organic chemistry

organic compound nomenclature

A

1-meth
2-eth
3-prop
4-but
5-pent
6-hex
7-hept
8-oct
9-non
10-dec

39
Q

organic chemistry

difference between unsaturated and saturated hydrocarbons

A

saturated: single bonds
unsaturated: double/triple bonds

40
Q

organic chemistry

hydroxyl functional group

A

R-O-H
alcohol

41
Q

organic chemistry

carboxyl functional group

A
  • carboxylic acid
    r-(o=c-o)-h
    *where r is bonded to the c atom
42
Q

organic chemistry

ester linkages`

A

-SINGLE bonded oxygen bonds to another hydrocarbon (cutoff!)
-r1(o=c-o)-r2
*where r1 is bonded to the c atom

43
Q

organic chemistry

halogens

A

-halogen atom (G17) bonds to hydrocarbon
- R-X, x= halogen

44
Q

organic chemistry

what is a structural isomer

A
  • same molecular formula, but different structure
  • similar chemical properties but different physical properties
45
Q

organic chemistry

what is an addition reaction

A

-diatomic molecules added across double/triple bond
- becomes more saturated (e.g. double–>single)

46
Q

organic chemistry

what is a substitution reaction

A
  • atom replaces another atom in a molecule
  • often require the presence of light
47
Q

organic chemistry

what is an elimination reaction

A
  • molecule is removed, create double bond
  • water or hydrogen halide is commonly produced
    -(reverse addition)
48
Q

organic chemistry

what is an esterification reaction

A
  • water is eliminated (created) to make an ester
  • carboxylic acid + alcohol = ester + water
49
Q

organic chemistry

what is a combustion reaction

A
  • hydrocarbon or alcohols react with oxygen to produce CO2 and water
50
Q

organic chemistry

polar vs non-polar structure

A

polar = asymmetrical
nonpolar = symetrical

51
Q

what is the haber process

A

production of ammonia
n2 + 3h2 <-> 2NH3

52
Q

what does shift left/right mean

A

right: more products formed
left: more reactants formed

53
Q

le chatliers principle: temperature

A

increase: shift endothermic right, exothermic left
decrease: shift endothermic left, exothermic right

54
Q

le chatlier’s principle: concentration

A

shift right. (add to right): increase reactant, decrease product
shift left (add to left): increase product, decrease reactant

55
Q

le chatlier’s principle: volume/pressure

A

increase: shift to side w more moles of gases
decrease: shift to side w less moles of gases

56
Q

what is the equilibrium constant?

A

kc, for aA+bB=cC+dD
[C]c[D]d/[A]a[B]b
affected by temperature

57
Q

kc generalizations

A

kc >1 = products favoured
kc = 1, relatively the same concentration
kc < 1, reactants favoured

58
Q

what is a bronsted-lowry acid and base

A

acid: proton donor
base: proton acceptor

59
Q

what does polyprotic mean

A

conjugate base can continue to give away protons (H+), can be determined by # of H’s

60
Q

equilibrium position in relation to acid base strength

A

check side with stronger acid/base, weaker side will be favoured

61
Q

conjugate acid/base pairs + equilibrium position

A
  • all reactions have two conjugate acid-base pair
    differ by one proton
  • if acid higher than base, favours products (>50%)
  • if acid lower than base, favours reactants(<50%)
62
Q

what is an amphiprotic substance

A

can act as an acid or a base

63
Q

what is a buffer

A

-mixture of weak acid and conjugate base
- addition of acid/base will be neutralized to water, by the opp (acid/base, base/acid)

64
Q

what is the equivalence point

A

same # of mole of titrant added a tere were moles of sample
>7 = SB-WA
<7 = SA-WB
=7, SA-SB

65
Q

ph and h3O formula

A

ph=-log[H3O]
[H3O]=10^-ph
responsible for acidic properties

66
Q

pOH and OH formula

A

pOH=-log[OH]
OH=10^-pOH
responsible for basic properties

67
Q

what is Kw

A

-equilibrium constant for ionization of water
-kw=1.00x10^-14. (=[h3O][OH])

68
Q

what is Ka

A
  • equilibrium constant for reaction of acid with water
    Ka = [H3O][A-]/HA (prod/reactant)
69
Q

what is Kb

A
  • equilibrium constant for reaction of base with water
  • kb = [OH][HA]/[A] (prod/reactant

flash (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions