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The DAT > Chem Equations > Flashcards

Chem Equations Flashcards

1
Q

Energy of a quantum?

A

E=hf, where h=planck’s constant=6.626e-34 J/s; and f=freq of radiation

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2
Q

angular momentum?

A

L=mvr

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3
Q

kinetic energy?

A

K=mv^2/2

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4
Q

angular momentum using classical physics and planck’s constant

A

L=nh/2pi; where n=principal quantum number, h=planck’s constant=6.626e-34

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5
Q

energy of an electron

A

E=-Ry/n^2; where Ry=Rydberg constant=2.18e-18 J/electron

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6
Q

electromagnetic radiation of a photon emitted by an excited electron

A

Ep=hc/lambda
where h=planck’s constant=6.626e-34, c=velocity of light in a vacuum=3.00e8 m/s, lambda is the wavelength of the radiation

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7
Q

Lyman series

A

Final E level=1=>emits UV light

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8
Q

Balmer series

A

Final E level= 2 => emits UV and visible light

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9
Q

Paschen series

A

Final E level= 3 => emits IR light

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10
Q

energy of an electron

A

Ee=Ry(1/ni^2-1/nf^2)

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11
Q

Energy of electron and photon?? lol idk

A

E=hc/lambda= -Ry(1/ni^2-1/nf^2)

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12
Q

max number of electrons in an electron shell

A

2n^2

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13
Q

number of e-s within a subshell

A

4l+2

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14
Q

formal charge

A

V-1/2Nbonding-Nnonbonding

where V=number of VEs, or V-#sticks-#dots

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15
Q

dipole moment of a polar molecule

A

mu=qr, where q= charge mag; r=distance bw two partial charges

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16
Q

moles exchanged in a rxn

A

M^n+ne- –> M

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17
Q

charge of an electron

A

1.6e-19 C

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18
Q

charge of one moles of e

A

1.6e-19 x 6.02e23 = 96 487 C/mol e-

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19
Q

1 Farad

A

96 487 C or J/V; ~ 10e5

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20
Q

Boiling point elevation

A

extent to which a bp of a sol’n is raised relative to that on the pure solvent;
dTb=i Kb m; i = van’t Hoff factor;

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21
Q

osmotic pressure

A

pi= i M R T; i= van’t Hoff factor; M= molarity; R=ideal gas constant; T= temp in K

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22
Q

Raoult’s law

A

Pa=XaPa and Pb= XbPb; applies only when the attraction between a & b is equal to the attraction between a & a and b and b

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23
Q

atm to Pa to torr to mmHg

A

1 atm = 10e5 Pa= 760 torr = 760 mmHg

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24
Q

Boyle’s law

A

P1V1=P2V2

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25
Q

Charles law

A

V1/T1=V2/T2

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26
Q

Avagadro’s principle

A

n1/V1=n2/V2

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27
Q

ideal gas law

A

PV=nRT

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28
Q

1 mole gas occupies 22.4L under STP (273 K, 1 atm)

A

ya

29
Q

moles transferred by electrochem cel

A

i t = n F
where t= time is secs
n= # of moles of e-s
F = faraday constant (10e5 C)

30
Q

electromotive force

A

Ecell = Ered + E* ox

31
Q

Gibbs free e of a cell

A

dG= -n F E*cell

32
Q

nFE*cell = RTlnKeq

A

ya

33
Q

Nernst eq

A

for non-standard conditions; Ecell= E*cell- (RT/nF)(ln Q), where Q = ([C]^c[D]^d)/([A]^a[B]^b)

34
Q

rate of reaction

A

-[dR]/t or [dP]/t

35
Q

rate for forward, irreversible rxn aA+bB–> cC+dD

A

rate= k [A]^x[B]^y

36
Q

overall rxn rate

A

sum of orders (x+y)

37
Q

0-order rxn rate, conc A at time t, half life

A

rate = k, conc A = [A]=[A0]-(k0)(t), t1/2 = 1/2*A0/k0

38
Q

1st-order rxn rate, conc A at time t, half life

A

rate = k[A] or k[B]; conc a time t = [At] = [A0] e^(-kt); t1/2= ln2/l = 0.693/k

39
Q

2nd order RR

A

k[A]^2, k[B]^2 or k[A][B]

40
Q

collision theory reaction rate:

A

rate = fZ, where Z is total # of collisions, f is the fraction of effective collisions

41
Q

heat absorbed or released in a rxn

A

q=mcT

42
Q

change in heat (enthalpy) at constant pressure

A

heat rxn= Hprod-Hreact

43
Q

standard heat of formation is for ONE MOLE of product–product must have ONE in front of it in a rxn–even if there are fractions

A

ya

44
Q

standard heat of rxn

A

sum of Hfprods - sum of Hfreactants

45
Q

standard entropy change of a rxn

A

sum of Sprod-sum of Sreactants

46
Q

entropy in the universe

A

must remain constant– Suni= Ssystem+Ssurroundings > 0

47
Q

Free E of a system

A

dG= H-TS, where T - abs temp in Kelvin

48
Q

standard free e

A

stGrxn= sum of Gfprods-sum of Gf react at 25 C, 1 atm

49
Q

G with Keq

A

G=-RTlnKeq

50
Q

G rxn not at eq

A

G= stG + RTlnQ, where stG= -RTlnKeq

51
Q

Keq

A

Keq= [C]^c[D]^d/[A]^a[B]^b

52
Q

le chatelier’s principle

A

increase in pressure–>favours side of rxn with fewest moles of gas cules; increase in volume–> eq shifts so more prod of substances with highest amount of moles

53
Q

Ion product

A

for rxn AmBn–> mA(aq) + nB (aq),

Qsp= [A]^m[B]^n

54
Q

solubility prod constant

A

Ksp = [A]^m[B]^n, in a saturated sol’n; varies with temp,

55
Q

describe the relationships bw Ksp and Qsp

A

if a salt’s:
Ksp=Qsp, system is at equil, saturated
Ksp>Qsp, system is undersat
Ksp

56
Q

conv of cal to joule

A

1 cal = 4.184 J

57
Q

specific heat gained or lost by a substance

A

Q=mcT=mc(Tf-Ti)

58
Q

specific heat capacity for water

A

c= 1 cal/g K = 1cal/g C = 4.184 j/g K

59
Q

heat of transformation

A

Q=m Hl where Hl is the latent heat–i.e. amount of heat needed for 1 kg of substance to change phase–>temp remains constant during phase changes

60
Q

heat of fusion

A

Hf–> for solid liquid

61
Q

heat of vaporization

A

Hv: for liquid gas

62
Q

freezing point depression

A

dTf= i Kp M where Kp=proportionality constant for a given solvent; m=molality (mol solute/ kg solvent); i -van’t Hoff factor–>accounts for number of particles that dissociate from original ‘cule

63
Q

dalton’s law

A

partial pressure’s – Pt= Pa + Pb + Pc… + Pz

64
Q

Partial p of a gas

A

Pa= Ptot Xa

65
Q

average KE of gas?

A

3/2 kT where k = boltzmann constant, T in kelvin

66
Q

rate pf gas diffusion

A

r1/r2= sqrt (MM2/MM1)– under isothermal and isobaric conditions

67
Q

Kw

A

[H][OH] = 1e-14

68
Q

percent ionization

A

ionized acid conc @eq/ initial conc of acid x 100

69
Q

review nuclear decay

A

ya

The DAT (22 decks)

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