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mcat > Gen Chemistry 2 (complete) > Flashcards

Gen Chemistry 2 (complete) Flashcards

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MCAT flashcards
1
Q

in the first law of thermodynamics, when is work negative and when is work positive

A

work done ON a system is positive and work done BY the system is negative

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2
Q

what are the three kinds of heat exchange and explain

A

convection: fluid movement caused by hotter portions rising and cooler fluid sinking
radiation: light colors radiate and absorb less while dark colors absorb and radiate more
conduction: high energy molecules collide with neighbors and give energy until the energy is equally spread out

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3
Q

what equation is used to do calorimeters questions

A

q=mc∆T, possibly q=C∆T

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4
Q

what is heat capacity

A

amount of energy a system must absorb to change temperature

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5
Q

what is the first law of thermodynamics

A

energy can neither be created nor destroyed

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6
Q

what is the formula for specific heat capacity

A

q=mc∆T

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7
Q

what is the pressure-volume work equation

A

PV Work = P∆V

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8
Q

what is the second law of thermodynamics

A

heat cannot be changed completely into work in a cyclical process

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9
Q

can heat be seen to flow from cold to hot object spontaneously?

A

no, it goes from cold/hot to mixed

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10
Q

what is the third law of thermodynamics

A

pure crystalline substances at absolute zero have an entropy of zero

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11
Q

where on the graph is pv work?

A

area under the curve

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12
Q

zeroth law of thermodynamics

A

everything tends to move toward thermal equilibrium with everything else

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13
Q

calorimeter

A

device used to calculate enthalpy change

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14
Q

what does delta H mean? give the equation of delta H

A

enthalpy change; delta H = products - reactants

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15
Q

what is enthalpy?

A

energy contained within chemical bonds

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16
Q

in an energy graph which part is the delta H? picture a graph with a dotted line with reactants in a higher part than products. the dotted line cuts through the middle of both

A

delta H is the distance between the products and dotted line

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17
Q

what is delta S

A

entropy

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18
Q

define entropy

A

a measure of the randomness or disorder in a system

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19
Q

what is delta G

A

gibbs free energy

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20
Q

what is gibbs free energy

A

the amount of “free” or “useful” energy available to do work

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21
Q

a 100g sample of which of the following elements will contain the least number of moles?
Li
Ba
Ca
Na

A

Ba: largest molar mass means least number of moles

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22
Q

how to convert celsius to Kelvin

A

Tc +273 =Tk

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23
Q

if delta S > 0, what does that mean for the randomness/disorder

A

disorder increases, releasing energy into the system that can be used to do work

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24
Q

if delta S < 0, what does that mean for the randomness/disorder

A

disorder decreases, taking energy from the system, decreasing energy available to do work

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25
Q

in gibbs free energy, what does +deltaG and
-deltaG mean?

A

+deltaG: nonspontaneous process, energy is required
-deltaG: spontaneous process, energy is made available

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26
Q

pH vs pka definition

A

pH: measure of H+ ions in the solution; it can change as the solution composition changes
pKa: does not change unless the compound itself changes

27
Q

if pH is greater than pKa, which is more, acid or base? what about the solute?

A

base; solute acts as an acid

28
Q

if pH is less than pKa, which is more, acid or base? what about the solute?

A

acid; solute acts as a base

29
Q

arrhenius acids produce what kind of solution? arrhenius bases produce?

A

acids produce H+ in solution, bases produce OH-

30
Q

brønsted-lowry acids donate what
what do bases do

A

acids donate H+ and bases accept them

HCl + SO4^-2 —–> Cl- + HSO4-
acid. base. conjugated
base acid

31
Q

lewis acid does what with electrons
lewis base does what with electrons

A

lewis acid: accept electrons
lewis base: donate electrons

32
Q

what can amphoteric substances do? give 2 examples

A

can act as either an acid or base

ex. H2O or HSO4-

33
Q

how do you calculate pH
make an example of trying to calculate the pH 1
pH 7?
pH 12?

A

pH 1= 1.10^-1 m [H+]
pH 7= 1.10^-7 m [H+]
pH 12= 1.10^-12m [H+]

34
Q

which of these will dissociate in water? strong acid
strong base
weak acid
weak base

A

both strong acid and base will dissociate 100% in water
both weak acid and base will only partially dissociate

35
Q

what are some examples of strong acids

A

HI, HBr, HCl, HNO3, HClO4, HClO3, H2SO4, H3O+

36
Q

what are some examples of strong bases

A

NaOH, KOH, LiOH etc
NH2-, H-, Ca(OH)2, Si(OH)2, Ba(OH)2, Na2O, CaO

37
Q

how do you know if it is a strong acid

A

if it is an ionic compound with H+ as the cation, it is a strong acid

38
Q

how do you know if it is strong base

A

if it has OH, it is a strong base

39
Q

henderson-hasselbach equation

A

pH=pKa + log [A-]/[HA]

40
Q

what is the henderson-hasselbach equation used for

A

used to determine the relationship between acids and bases

41
Q

what is the salt of a weak acid

A

conjugate base plus a cation

42
Q

what is the salt of a weak base

A

conjugate acid plus an anion

43
Q

what is titration

A

process of adding acid of a known concentration to base of an unknown concentration (or vice versa) to figure out the unknown concentration

44
Q

how does a graph look for Strong acid/Strong base? think how it looks on pH

A

starts at low Ph and ends at a high pH

45
Q

how does a graph look for Strong Base/strong acid? think how it looks on pH

A

starts at high pH and ends at low pH

46
Q

how does a graph look for weak acid/weak base? think how it looks on pH

A

starts mid-low pH and ends at high

47
Q

how does a graph look for weak base/weak acid? think how it looks on pH

A

starts mid high and ends mid low

48
Q

if a reaction is at max entropy, what does that mean?

A

it is at equilibrium

49
Q

equation of Ka

A

Ka = [H+][A-]/[HA]

50
Q

equation of Kb

A

Kb= [OH-][HA]/[A-]

51
Q

is CO2 polar or non polar

A

non polar
there is even distribution

52
Q

in the case of the same liquid being in two different containers, and the pressure is measured at 10cm deep, how does the pressure differ

A

it doesn’t because the height is the same, doesn’t matter the shape
and the liquid is the same

53
Q

what is boyles law

A

P1V1=P2V2

54
Q

what is charles law

A

V1/T1=V2/T2

55
Q

how do you find the number of neutrons in an element

A

atomic mass-atomic number

56
Q

what is the volume at STP

A

22.4L
1mole of gas = normal volume

57
Q

what is visible light in

A

400-700nm

58
Q

what wavelength do you need to see bacteria

A

400-700

59
Q

list the wavelengths from big to small
low frequency to high

A

radio
micro
IR
visible
UV
xray
gamma

60
Q

dipole movement

A

separation of partial charges across polar bonds

61
Q

if you are given Radium-226, how would it change with alpha decay
(note: atomic number is 88)

A

it would go from 226/88 Ra to 222/86 Rn
bc alpha means lose 4 on top and 2 on bottom

62
Q

if you are given Radium-226, how would it change with beta decay
(note: atomic number is 88)

A

it would go from 226/88 Ra to 226/87 Fr
bc beta means the top number stays the same but the atomic number/bottom decreases by 1 (the element does change bc atomic number changed)

63
Q

if you are given Radium-226, how would it change with gamma emission
(note: atomic number is 88)

A

it would go from 222/88 Ra to 226/88 Ra
it would stay the same bc no nuclear conversion or release of energy is happening

64
Q

if Ka is given and you are asked to find Kb, what do you do?

A

14-Ka=Kb

mcat (13 decks)

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