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MCAT > Physics and Chem Section > Flashcards

Physics and Chem Section Flashcards

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MCAT flashcards
1
Q

When calculating the density of a volatile liquid, must take what into account

A

some will evaporate – so will lose mass

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2
Q

Mass % of a solute * Density =

A

(Mass Solute/Mass Soln)*(Mass Soln/Vol Soln) = Mass Solute/Vol Soln

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3
Q

How to convert from grams or moles of a gas to get to liters of an ideal gas at STP?

A

22.4 Liters of gas / 1 mol gas (so would need to convert grams of gas to mols first if given grams)

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4
Q

Molecular Formula vs Empirical Formula

A

Molecular Formula is the actual mole ratio of the elements within the compound. Empirical Formula uses the smallest whole number ratio of the atoms in each compound.

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5
Q

How to calculate empirical formula

A

Assume 100–gram sample so the percentages can easily be changed into mass figures then convert mass into moles (using atomic masses of each element) the empirical formula is then the whole number ratio of these mol values

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6
Q

How to convert between molecular and empirical formulas

A

Multiply the empirical formula by the whole number ratio of the molecular mass to the empirical mass

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7
Q

What is a combustion reaction?

A

Hydrocarbon + Excess Oxygen ––––combusted–––> Carbon Dioxide + Water Vapor CxHy + O2 –––> CO2 + H2O (Hydrocarbon is oxidized)

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8
Q

Molality (m)

A

Moles Solute / Mass Solvent (kg)

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9
Q

Which of the following are affected by temperature changes? Molarity Molality Mass Percent”

A

Molarity = IS affected Molality = IS NOT affected Mass Percent = IS NOT affected

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10
Q

Mass Percent (in soln)

A

Mass Solute / Mass Solution *100%

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11
Q

Trick for calculating dilution

A

Recognize that total moles of a solute remain constant when a solvent is added, so M*V remains constant: MiVi = MfVf

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12
Q

What is a simple dilution?

A

Addition of pure solvent

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13
Q

What is Beer’s Law? –idea behind it –equation for it –trick for solving problems

A

States that you can pass electromagnetic radiation through a solution and the solution may absorb some of the light – the light absorbed will be a specific wavelength range and the absorbance intensity will vary directly with the concentration of the solute:

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14
Q

What is Beer’s Law? –equation for it

A

Abs = ε*C*l where ε = a constant for the soln at λmax C = [solute] l = width of cuvette (length of pathway through which light passes)

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15
Q

What is Beer’s Law? –trick for solving problems

A

Absi * Vi = Absf*Vf

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16
Q

the limiting reagent is the reactant with _______________

A

the lowest ratio of actual moles to needed moles

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17
Q

What are the solubility rules?

A

(1) Most salts containing alkali metal cations (Li+, Na+, K+, Cs+, Rb+) and Ammonium (NH4+) are water soluble (2) Most nitrate (NO3–) salts are water–soluble (3) Most salts containing halide ions (Cl–, Br–, I–) are water–soluble (except with heave metals such as Ag+ and Pb2+) (4) Most salts containing Sulfate anions (SO42–) are water–soluble (5) Most hydroxide anion (OH–) salts are only slightly water–soluble. (KOH ad NaOH are substantially soluble, while Ca(OH)2, Sr(OH)2, and Ba(OH)2 are fairly soluble) (6) Most carbonate anion (CO32–), chromate anion (CrO42–), phosphate anion (PO43–), and sulfide anions (S2–) salts are only slightly water–soluble

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18
Q

CaCO3 is a(n) ____________

A

BASE

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19
Q

In composition reactions, what is happening (and how is entropy affected)

A

Reactants combining to form a product: More bonds formed, so entropy decreases

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20
Q

In decomposition reactions,what is happening (and how is entropy affected)

A

Reactants decompose to form multiple products: More bonds broken = entropy increases

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21
Q

Which atom (or compound) is the reducing agent (reductant) and which is the oxidizing agent (oxidant)

A

Atoms losing electrons = reducing agent (reductant) Atoms gaining electrons = oxidizing agent (oxidant)

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22
Q

Loss of Electrons in a reaction = a(n) _______ Gain of Electrons in a reaction = a(n) ______

A

Loss of Electrons = Oxidation Gain of Electrons = Reduction LEO the lion goes GER

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23
Q

In combustion reaction, oxygen serves as the _______

A

oxidizing agent

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24
Q

Oxidation state of an atom an be determined by ________

A

looking at bonds it forms with less electronegative atoms (gives it a –1 for every bond) and bonds it forms with more electronegative atoms (gives it a +1 for every bond)

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25
Q

general rules for assigning oxidation states

A

O = –2 (except in molecular oxygen and peroxides) H = +2 (except in molecular hydrogen and hydrides) Halides = –1 (except when they are a central atom in an oxyacid)

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26
Q

1/5

A

0.2

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27
Q

1/6

A

0.1166

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28
Q

1/7

A

0.143

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29
Q

1/8

A

0.125

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30
Q

1/9

A

0.111

31
Q

1/11

A

0.091

32
Q

1/12

A

0.083

33
Q

conduction vs convection

A

conduction = transfer of heat through direct contact convection = transfer of heat through a liquid or gas medium

34
Q

sublimation

A

solid –––––> gas

35
Q

giga =

A

10^9

36
Q

mega =

A

10^6

37
Q

deci =

A

10^ –1

38
Q

centi =

A

10^ –2

39
Q

milli =

A

10^ –3

40
Q

micron =

A

1 micron = 10^ –6 meters

41
Q

Angstrom =

A

1 Angstrom = 10^ –10 meters

42
Q

pico =

A

10^ –12

43
Q

fempto =

A

10^ –12

44
Q

calorie to joule conversion

A

1 calorie = 4.18 Joules

45
Q

kilogram to pound conversion

A

1 kg = 2.2 pounds (on earth)

46
Q

liter to meter conversion

A

1000 liters = 1 cubic meter

47
Q

Mile to meter conversion

A

1 mile = roughly 1600 meters

48
Q

foot to meter conversion

A

1 meter is a little over 3 feet

49
Q

inch to cm conversion

A

1 inch = roughly 2.5 cm

50
Q

**Important Trig function to remember**

A

cos^2(theta) + sin^2(theta) = 1

51
Q

cos 0 =

A

1

52
Q

cos 30 =

A

sqrt(3) / 2 = 0.86

53
Q

cos 45 =

A

sqrt(2) / 2 =0.71

54
Q

cos 60 =

A

1/2 =0.50

55
Q

cos 90 =

A

0

56
Q

sin0 =

A

0

57
Q

sin 30 =

A

1/2 =0.50

58
Q

sin 45 =

A

sqrt(2) / 2 =0.71

59
Q

sin 60 =

A

sqrt(3) / 2 =0.86

60
Q

sin 90 =

A

1

61
Q

tan =

A

sin/cos =opp/adj

62
Q

What is the kinematic equation to use when: you don’t have Vfinal? (assume all are in x direction)

A

Δx = viΔt + 1/2 a(Δt)^2

63
Q

What is the kinematic equation to use when: you don’t have dx(displacement of x)? (assume all are in x direction)

A

vf = vi + a(Δt)

64
Q

What is the kinematic equation to use when: you don’t have a? (assume all are in x direction)

A

Δx = (1/2)*(vi + vf)*Δt

65
Q

What is the kinematic equation to use when: you don’t have t? (assume all are in x direction)

A

(vf)^2 =(vi)^2 + 2aΔx

66
Q

Without air resistance, a ball will fall _____ meters in 1 second, _____ meters in 2 seconds, and so forth (_______)

A

Will fall 5 meters in 1 second and 20 meters in 2 seconds (and 80 meters in 4 seconds) Δy = 5t^2 *assuming starts with zero velocity

67
Q

Estimate (disregarding air resistance) the velocity of a ball falling after 1 second, 2 seconds, etc.

A

Velocity = 10Δt *assuming starts with zero velocity so after 1 second, v = 10 m/s 2 seconds, v = 20 m/s 3 seconds, v = 30 m/s and so on

68
Q

Calculate how much time (disregarding air resistance) it will take a ball to reach the top given an initial velocity

A

Δt = vi / 10

69
Q

Throwing a projectile: Calculate the height the projectile travels

A

h = (viy)^2 / 10 or (viy)^2 /g

70
Q

Throwing a projectile: Calculate the time it takes the projectile to reach the top

A

t = viy / 10 or t = viy / g

71
Q

Calculate the range of a projectile

A

r = 2voxvoy / g r = (vo)^2 sin2Θ / g

72
Q

When does a projectile have maximum range? What is the formula for its range in that case?

A

when Θ = 45 degrees r = (vo)^2 sin(90) / g = (vo)^2 / g

73
Q

What is the relationship between r and f at given thetas (from the horizontal): 30 degrees 45 degrees 60 degrees”

A

30 degrees: r/h = 6.7 45 degrees: r/h = 4 60 degrees: r/h = 2.4

MCAT (14 decks)

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