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MCAT general Chem > Equations > Flashcards

Equations Flashcards

1
Q

Plank’s frequency relation

A

E = h(f or nu)

E=energy
h= Plank’s constant (6.63 x 10^-34 Js)
f=frequency

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2
Q

What equation is similar to Plank’s frequency relation?

A

c/v=wavelength x frequency (v or nu)

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3
Q

When would Plank’s frequency relation be used?

A

To calculate energy or frequency

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4
Q

Angular momentum equation

A

L=nh/2(pi)

n=principal quantum number
h=Plank’s constant

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5
Q

Plank’s constant

A

6.63 x 10^-34 Js

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6
Q

When would angular momentum of an electron around a hydrogen be used?

A

Quantized by higher principle number, higher momentum

Larger principle quantum numbers have higher momentum

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7
Q

Energy of an electron equation

A

E=-RH/n^2

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8
Q

When would the energy of an electron be important?

A

Energy of electron is directly proportional to the principle quantum number
Because of negative sign, larger number gets closer to zero, larger

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9
Q

Rydberg unit of energy

A

2.18 x 10^-18 J/electron

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10
Q

Avagadro’s number

A

6.02 x 10^23
Measure of things - usually measures a number of atoms within a mass number
1 mol=6.02 x 10^23 atoms= # amu
The units of a mol

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11
Q

Electromagnetic energy of a photon equation

A

E=hc/(wavelength) or

-RH[1/n^2-1/n^2]

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12
Q

Speed of light (c)

A

3 x 10^8 m/s

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13
Q

Max number of electrons in a shell

A

2n^2

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14
Q

Values of l

A 
Subshell
0=s
1=p
2=d
3=f
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15
Q

Max number of electrons in a subshell

A

4l + 2

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16
Q

Max value of l

A

0 to n-1

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17
Q

ml

A

Orbital within subshell

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18
Q

Max electrons in a orbital

A

2e

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19
Q

Values of ml/orbitals per l

A

any l has 2l +1 values of ml

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20
Q

Orbitals/ml per principle number

A

n^2

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21
Q

Values of ms

A

+1/2, -1/2

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22
Q

How to determine which subshell is lower

A

n +1

If same, lower n will fill first

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23
Q

Values of ml

A

between -l and +l

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24
Q

Percent composition

A

All of them= 1

Each one’s mass number amount= given atomic weight

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25
Q

1 amt =

A

760 Torr = 760 mmHg = 101.325 kPa

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26
Q

STP

A

273 K
1 atm
For gas law calculations

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27
Q

Standard conditions

A

298 K
1 M
For entropy, enthalpy, Gibb’s free energy, and electromotive forces

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28
Q

Ideal gas law

A

PV=nRT

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29
Q

R

A

Ideal gas constant
8.21 x 10^-2 Latm/molK
or 8.314 J/molK

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30
Q

How much does 1 mol of ideal gas occupy?

A

22.4 L

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31
Q

Density equation

A

=m/V = PM/RT

32
Q

Combined gas law

A

PV1/T1 = PV2/T2

33
Q

When would the combined gas law be used?

A

When the moles stay constant, but need to find the other factor

34
Q

How to find density from combined gas law?

A

Substitue V1= 22.4 L and use STP to compare to current

Then divide mass/new volume

35
Q

How to find molar mass from combined gas law?

A

Used combined gas to find V at STP
Divide weight by newfound liter amount
Multiply g/L by ideal gas volume = g/mol
Density at STP x volume of one mol

36
Q

Avagadro’s principle

A

n/V=k
n1/V1=n2/V2

k is a constant

37
Q

Gibb’s free energy equation

A

Delta G= Delta H- TDelta(S)

38
Q

Percent by mass

A

mass of solute/mass of solution x 100

39
Q

Mole fraction

A

mol of A/mol of all species

40
Q

Molarity

A

mol solute/L solution

41
Q

p value=

42
Q

Ka

A

[H3O=]{A-]/[HA]

43
Q

Kb

A

[B+][OH-]/[BOH]

44
Q

Faraday’s constant

A

10^5 C/mol e-

45
Q

Electrodeposition equation

A

mol M=It/nF

n=oxidation state

46
Q

Boyle’s Law

A

PV=k

PV=PV

47
Q

Charles’s Law

A

V/T=k

V/T=V/T

48
Q

Gay-Lussac’s Law

A

P/T=k

P1/T1=P2/T2

49
Q

Dalton’s Law of Partial Pressures

A

Ptotal=PA + PB +PC …

50
Q

Partial pressure equation

A

PA=XA(PT)

XA=mol of gas A/total moles of gas

51
Q

Vapor pressure

A 
[A]= kH x Pa 
[A]1/P1=[A]2/P2= kH

[A]=concentration
kH=Henry’s constant
PA=partial pressure of A

52
Q

Average kinetic energy of a gas

A

KE=1/2mv^2=(3/2)kBT

kB=Boltzmann constant

53
Q

Boltzmann constant (kB)

A

1.38 x 10^-23 J/KT

54
Q

Root-mean-square speed (u rms)

A

u rms= Square root (3RT/M)

R=ideal gas constant
M=molar mass in kg/mol

55
Q

R (Ideal gas constant)

A

8.314 J/Kmol

56
Q

Graham’s law

A

r1/r2=Square root(M2/M1)

Ex. A gas that has a molar mass 4x of another, it will travel half as fast

57
Q

Van der Waals Equation of State

A

(P +n^2a/V^2)(V-nb)=nRT

ab=constants for each gas

58
Q

a constant

A

Corrects for attractive forces (smaller for smaller less polarizable molecules and largest for polar moleucles)

59
Q

b constant

A

Corrects for volume of molecules due to size

60
Q

Standard electromotive force (emf)

A

E(cell)=E(red,cathode)-E(red,anode)

61
Q

Do you multiply cell potentials when coming up with net reactions?

62
Q

Delta G and emf

A

Delta G= -nFEcell
n=mols of electrons exchanged
F=Faraday constant
Ecell=standard emf

63
Q

Deviation from normal cell emf

A

Ecell=E(cell standard) - RT/nF (lnQ)

Q=reaction quotient

64
Q

Simplified deviation from normal cell emf

A

E cell=E(cell standard) -0.0592/n(logQ)

65
Q

Reaction quotient

A

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

Lower case is number in front

66
Q

Delta G equation

67
Q

Change in Free energy of electrochemical cell with varying concentration

A

Delta G= Delta G(standard) + RTlnQ

68
Q

Rate law

A

k[A]^x[B]^y

69
Q

Arrhenius equation

A

k=Ae^-Ea/RT

70
Q

Radioactive decay

A

[A]t=[A]e^-kt

71
Q

Concentration of Solution after dilution

72
Q

Normality

A

mols solute/kg solvent

73
Q

Boiling point depression expression

A

Delta(T)=iKbm
i=van’t Hoff factor=number of particles in which a compound dissociates (NaCl=2)
Kb=proportionality constant of the solvent
m=molality

Temperature in Kelvin

74
Q

Density of water

75
Q

Freezing point depression

A

Delta T f=iKfm

i=van t’Hoff
Kf=proportionality constant
m=molality

Temperature in Kelvin

MCAT general Chem (9 decks)

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