Mcat Equations

Front 1

Final Velocity

Back 1

Vƒ = Vo + at

Front 2

Final Velocity Squared

Back 2

v^2 = V0^2 +2ad

Front 3

Delta X

Back 3

Vot + 1/2at^2

Front 4

Newton's second Law

Back 4

F = ma

Front 5

Force of Gravity

Back 5

Fg = Gm1m2/r^2

Front 6

Centripetal Acceleration

Back 6

Ac = v^2/r

Front 7

Static Friction

Back 7

0 <= Fs <= µsFn

Front 8

Kinetic Friction

Back 8

Fk = µkFn

Front 9

Torque

Back 9

t = rfsinΘ

Front 10

Center of mass

Back 10

(m1x1 + m2x2) / m1 + m2

Front 11

Momentum

Back 11

mv

Front 12

Conservation of momentum

Back 12

m1v1i +m2v2i = m1v1f + m2v2f

Front 13

Potential Energy

Back 13

mgh

Front 14

Kinetic energy

Back 14

1/2mv^2

Front 15

Work

Back 15

FdcosΘ

Front 16

Young's Modulus

Back 16

Stress/Strain

(F/A)(△L/L)

Front 17

Shear Modulus

Back 17

Stress over strain

(F/A)/(△x/h)

Front 18

Bulk Modulus

Back 18

Stress over strain

(F/A)/(△V/V)

Front 19

Impulse

Back 19

I = Ft = △p

Front 20

Power

Back 20

P = Work/Time in watts

or

IV

Front 21

Hook's Law

Back 21

F = -Kx

Front 22

Potential energy of a spring

Back 22

U = 1/2kx^2

Front 23

Frequency of a spring

Back 23

f = (1/2π) squareroot (k/m)

Front 24

Period of spring

Back 24

T = 2π squareroot(m/k)

Front 25

Frequency of Pendulum

Back 25

f = (1/2π)squareroot(g/l)

Front 26

Period of Pendulum

Back 26

2π squareroot(l/g)

Front 27

Density

Back 27

p = m/v

Front 28

Buoyant Force

Back 28

Fb = pgv

p is density of fluid, v is volume displaced

Front 29

Continuity equation

Back 29

A1V1 = A2V2

Front 30

Bernoulli's equation

Back 30

P + 1/2pv^2 +pgh = a constant

P is pressure
p is density
v is velocity

Front 31

Intensity

Back 31

I = P/A

Front 32

Decibel System

Back 32

B = 10log(I/Io)

I0 = 1 x 10^-12

Front 33

Beat frequency

Back 33

|f1 - f2|

Front 34

Wave velocity

Back 34

f X wavelength

Front 35

Wave period

Back 35

1/f

Front 36

Frequency on string, open pipe

Back 36

f = nv/2L n=1,2,3,4...

Front 37

frequency on pipe that is closed

Back 37

f = nv/4L n=1, 3, 5

Front 38

Wavelength on string, open pipe

Back 38

λ = 2L/n n=1,2,3

Front 39

Wavelength on closed pipe

Back 39

λ = 4L/n n=1,3,5

Front 40

Doppler effect

Back 40

F = f'(V +- Vd)/(V +- Vs)

V is velocity of sound, 340 m/d

Front 41

Coulomb's Law

Back 41

F = Kq1q2/r^2 = qE

Front 42

Electric Field

Back 42

E = F/q = Kq1/r^2 = V/d

Front 43

Electric Potential Energy

Back 43

U = Fr = Kq1q2/r = qV = qEd

Front 44

Electric Potential (Voltage)

Back 44

V = U/q = Kq1/r = Ed

Front 45

Electric Field in between two plates

Back 45

E = V/d

d = distance between two plates

Front 46

Ohm's Law

Back 46

V = IR

Front 47

Resistance of wire

Back 47

R = pL/A

Front 48

Force on charge in magnetic field

Back 48

F = qvbsinΘ

Front 49

Force on wire in magnetic field

Back 49

F = iLbsinΘ

Front 50

Magnetic Field In a loop of wire

Back 50

B = µoI/2r

Front 51

Magnetic Field on straight .wire

Back 51

B = µoI/2πr

Front 52

Resistance of resistors in series

Back 52

Req = R1 + R2 + R3

Front 53

Resistance of resistors in parallel

Back 53

1/Req = 1/R1 + 1/R2 + 1/R3

Front 54

Capacitance of capacitors in series

Back 54

1/C = 1/C1 + 1/C2 + 1/C3

Front 55

Capacitance of capacitors in parallel

Back 55

C = C1 + C2 + C3

Front 56

Capacitance

Back 56

C = Q/V

or, by purely physical dimensions:

C = EoA/L

Front 57

AC voltage

Back 57

Vmax / squareroot of 2

Front 58

AC current

Back 58

Imax / squareroot of 2

Front 59

Binding Energy

Back 59

E = mc^2

Front 60

Snell's Law

Back 60

n1sinΘ1 = n2sinΘ2

Front 61

Index of refraction

Back 61

n = c/v

Front 62

Magnification

Back 62

M = -i/0

Front 63

total internal reflection

Back 63

n1sinΘ1 = n2sin90

Front 64

Image, Object, Focal Length

Back 64

1/i + 1/o = 1/f = 2/r

Front 65

Power of lens

Back 65

P = 1/f

Front 66

Energy of a photon, with work function

Back 66

E = hf - w

Front 67

Energy of principal quantum level for hydrogen

Back 67

E = -13.6 eV/n^2

n = principle quantum number

Front 68

Ideal Gas Law

Back 68

PV = nRT

Front 69

Dalton's Law of partial pressure

Back 69

P = Pa + Pb + Pc
P = XaP + XbP + XcP
Pa = XaP

Front 70

Raoults law

Back 70

Pa = Xa VPa

VPa = vapor pressure of pure a
Pa = partial pressure of A in solution

Front 71

Graham's Law of effusion

Back 71

Va/Vb = squareroot(Mb/Ma)

Front 72

Boiling Point elevation

Back 72

ΔTb = Kbm

m = molality

Front 73

Freezing Point Depression

Back 73

ΔTf = Kfm

m = molality, but be sure to check the K for SI values

Front 74

Osmotic Pressure

Back 74

π = iMRT

M is molarity

Front 75

pH

Back 75

-log[H+]

Front 76

pOH

Back 76

-log[OH]

Front 77

Kw

Back 77

=10^-14 = [H+][OH-]

Front 78

Ka

Back 78

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

Front 79

Kb

Back 79

[HB+][OH-]/B

Front 80

pKa + pKb

KbKa

Back 80

14

10^-14

Front 81

Henderson Hassalbalch equation

Back 81

pH = pka + log [conj base]/[acid]

Front 82

1st law of thermo

Back 82

U = Q - W

Front 83

Gibbs free energy

Back 83

ΔG = H - TΔS

Front 84

Standard Gibbs free energy as a function of Keq

Back 84

ΔG° = -RTlnKeq

Front 85

Gibbs free energy in a reaction already going (no longer standard conditions)

Back 85

ΔG = RTln(Q/Keq) (simplified)

ΔG = ΔG° + RTlnQ

if Q < Keq, then Q\Keq ratio is less than one, ln of decimal is negative, free energy is negative, thus spontaneous, and the reaction will proceed forward until equilibrium is reached

if Q > Keq, then ratio is more than one, and ln is positive, meaning free energy change is positive, meaning reaction will proceed in the reverse direction spontaneously (?) until the reaction is at equilibrium

If Q/Keq = 1, reaction is at equilibrium. ln of 1 is zero

Front 86

Standard GFE in a cell

Back 86

ΔG° = -nFE°cell

Front 87

Combination of equations concerning ΔG°

Back 87

ΔG° = -nFE = -RTlnKeq

nFE = RTlnKeq

Front 88

Relationship between E°cell and Keq

Back 88

E°cell = (RT/nF)lnKeq

Front 89

E°cell

Back 89

E°ox + E°red

Front 90

Ecell as a function of concentrations

(Nernst equation)

Back 90

Ecell = E°cell - (RT/nF)lnQ

Front 91

Faraday's constant

Back 91

The number of coulomb's in one mole of electrons
10^5 C per mole of electrons

Front 92

eV

Back 92

electron volt
the amount of energy acquired when one electron moves through one volt
A unit of energy
1 eV = 1.6 X 10-19 J

Front 93

Max number of stereoisomers with n chiral centers

Back 93

2^n

Front 94

Hardy weinberg equations

Back 94

P + q = 1
p^2 + 2pq + q^2 = 1

Front 95

Number of different gamete types

Back 95

2^n

n is number of heterozygous genes

Front 96

STP

Back 96

standard temperature and pressure
T = 273 K
P = 1 atm = 760 torr = 760 mmHg = 101 kPa

Front 97

Standard state conditions

Back 97

298 K
1 atm (1 barr)
1M solutions

Front 98

Isolated system

Back 98

Not mass nor energy can be transferred

Front 99

Closed system

Back 99

Mass cannot be transferred, but energy can

Front 100

Open system

Back 100

Both mass and energy can be transferred

Front 101

standard heat of reaction

Back 101

ΔH°rxn = ΔH°f products - ΔH°f reactants

Front 102

Ksp for
AgCl <--> Ag+ + Cl-

Back 102

[An+]^m[Bm-]^n

Front 103

Ksp for MX

Back 103

x^2

Front 104

Ksp for MX2

Back 104

4x^3

Front 105

Ksp for MX3

Back 105

27x^4

Front 106

Ksp for M2X3

Back 106

108x^5

Front 107

Rate Law for

aA + bB --> cC + dD

Back 107

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

x and y are determined EXPERIMENTALLY

rate law regards the concentrations of the REACTANTS

Front 108

how is k from rate law and Keq related?

Back 108

Keq = kf/kr

Front 109

Law of mass action

for aA + bB --> cC + dD

Back 109

No matter how many steps,

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

pure solids and liquids are not included in the equilibrium expression.

Front 110

Progress towards equilibrium:
1. Qc < Keq
2. Qc = Keq
3. Qc > Keq

Back 110

1. Reaction has not yet reached equilibrium
2. Reaction has reached equilibrium
3. Reaction has exceeded equilibrium

Front 111

Oxidation Number rules (the weird ones)
1. The oxidation number of halogens in a compound is -1, except when paired with...
2. The oxidation of hydrogen is -1 in compounds that are...
3. Oxygen has an oxidation number of -2, except when...

Back 111

1. something that has a higher electronegativity. Ex: HOCl, ox number of cl is +1
2. less electronegative than hydrogen. Ex: NaH, CaH2
3. paired with F, because it is more electronegative, or in peroxides like BaO2 in which the O has a -1 oxidation state

Front 112

Steps of Balancing Redox Reaction

Back 112

1. Separate two half reactions
2. Balance the atoms that are NOT H and O
3. Acidic solution --> Add H2O to balance the O atoms, add H+ to balance the H atoms
Basic Solution --> Add H2O and OH-
4. Balance charges of each half reaction with electrons.
5. Multiply each reaction by some integer so that electrons for both reactions are equal
6. Add the half reactions
7. Ensure Mass and Charge is Balanced

Front 113

Standard EMF

Back 113

E°red + E°ox

or

E°cath - E°anode

Front 114

Pascal's principle

Back 114

P1 = P2

F1/A1 = F2/A2