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chem 400 > exam 2 > Flashcards

exam 2 Flashcards

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1
Q

What is stoichiometry

A

The numerical relationships between chemical amounts in a balanced equation

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2
Q

What is the limiting reactant?

A

The reactant that limits the amount of product in a chemical reaction

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3
Q

What is the theoretical yield?

A

The maximum amount of product that can be made in a chemical reaction based on the amount of limiting reactant

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4
Q

What is the actual yield?

A

The amount of product actually produced by a chemical reaction

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5
Q

What is the percent yield?

A

The percentage of the theoretical tield that is obtained, is calculated as the ratio of the actual yield to the theoretical yield (Actual/Theo)x100=%

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6
Q

Solve for the excess (find a random example

A

did you get it right lmfao

moles of limiting reactant–> molar ratio of limiting and excess-> grams of excess -> (total amt of excess-amount used)= excess leftover

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7
Q

What is a solution

A

A homogeneous mixture between two substances

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8
Q

What is the solvent?

A

The majority component of the mixture

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9
Q

What is the solute

A

The minority component of the mixture

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10
Q

What is an aqueous solution?

A

One in which water acts as the solvent

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11
Q

What is a dilute solution

A

A solution that contains a small amount of solute relative to the solvent

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12
Q

What is a concentrated solution

A

A solution thar contains a large amount of solute relative to the solvent

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13
Q

What is Molarity

A

A common way to express solution concentration

M=amount of solute (in moles)/volume of solution (L of solution)

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14
Q

What is the equation to find out how much stock solution to use in certain concentrations?

A

M1V1=M2V2

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15
Q

What are electrolytes

A

The dissolved ions in electrolyte solutions act as charge carriers that allow the solution to conduct electricity

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16
Q

What is a strong electrolyte

A

Substances that completely dissociate into ions when they dissolve in water and result in solutions that are strong electrolyte solutions

ex. Soluble Ionic compounds

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17
Q

what are nonelectrolytes/ weak electrolytes

A

Compounds that do not (completely) dissociate into ions when dissolved in water are nonelectrolytes

ex. Covalent Compounds, Organic Compounds

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18
Q

What is a strong acid

A

An acid that completely ionizes in a solution

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19
Q

What is a weak acid?

A

An acid that does not completely ionize in water: this is represented by half arrows in the formula

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20
Q

What are weak electrolytes?

A

weak acids are weak electrolytes and only weakly conduct electricity

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21
Q

What does it mean when a compound is soluble or insoluble

A

if the compound dissolves in water it is soluble, if it does not, it is insoluble

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22
Q

Review the solubility rules

A
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23
Q

What is a precipitation reaction?

A

Reactions in which a solid or precipitate forms when we mix two solutions: only insoluble compounds form precipitates

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24
Q

What is the difference between molecular, complete ionic, and net ionic equations?

A

A molecular equation is an equation that shows the complete neutral formulas for each compound in the reaction as if they existed as molecules.

A complete ionic equations show all of the ions present as either reactants or products, strong electrolytes are represented as their constituent ions but weak electrolytes are not

Net ionic equations only show the species that actually change during the reaction

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25
Q

What is an acid base reaction

A

A reaction where an acid reacts with a base and the two neutralize each other, producing water and an ionic compound (a salt)

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26
Q

What is a gas-evolution reaction?

A

a gas forms

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27
Q

What are the Arrhenius definitions of Acids and Bases

A

Acids are substances that produce H+ ions in an aqueous solution

Bases are substances that produce OH- ions in an aqueous solution

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28
Q

What are some strong acids?

A

HCI, HBr, HI, HClO4, HNO3, H2SO4 (only the first H+ lost is strong)

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29
Q

What are some common weak acids?

A

Formic acid (HCHO2), Acetic Acid (HC2H3O2), Hydrofluoric acid (HF)

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30
Q

What are some strong bases

A

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Ca(OH)2, group 1 metals, Mg(OH)2, Sr(OH)2, Ba(OH)2, group 2 metals

31
Q

What are some weak bases?

A

Ammonia NH3

32
Q

What is a titration?

A

A titration is when a compound of a known concentration (known as the titrant) is reacted with a compound of unknown concentration but known volume (the analyte). The titrant is added to the analyte until the moles of titrant=the moles of analyte (this is the equivalence point. It is visualized by a color change)

33
Q

What is the equivalence point in a titration?

A

the point in the titration when the number of moles of OH- added equals the number of moles of H+ initially in the solution

34
Q

What are the reactants that under-go intermediate stages of gas evolution

A

Sulfides–>H2S

Carbonates and bicarbonates: (CO3^2-, HCO3)–> intermediate: H2CO3—> H20(l) + CO2(g)

Sulfites and bisulfites: (SO3^2-, HSO3)–> Intermediate: H2SO3—> H20 (l) +SO2

Ammonium: (NH4)–> Intermediate: (NH4OH)–> H20 (l) +NH3 (g)

35
Q

What are redox reactions?

A

Reactions in which electrons transfer from one reactant to the other. Many of these involve reactions with oxygen, nonmetals and metals, and with nonmetals

36
Q

What is oxidation?

A

The loss of electrons

37
Q

What is reduction?

A

The gain of electrons

38
Q

What is the oxidation state?

A

A number given to each atom based on the electron assignments, it is the “chatge” ot would have if all shared electrons were assigned to an atom with the greatest attraction for those electrons

39
Q

What are the rules for Oxidation states? (in order)

A
  1. The oxidation state of an atom in a free element is 0
    ex. Cu (ox=0), Cl2 (ox=0)
  2. The oxidation state of a monoatomic ion is equal to its charge
    ex. Ca2+ (ox=+2) Cl-(ox=-1)
  3. The sum of the oxidation states of all atoms in:
    • A neutral molecule or formula unit is 0
      ex. H20 (2x(ox of H) +1x(ox of O)= 0
    • An ion is equal to the charge of an ion
      ex. NO3- (1x(ox of N)+ 3x(ox O)= -3
  4. In their compounds metals have positive oxidation states
    - Group 1A is always +1
    -Group 2A is alwaus +2
  5. The oxidation states of nonmetals are assigned due to the table
40
Q

What is the oxidation state of Fluorine

A

-1

41
Q

What is the oxidation state of Hydrogen

A

+1

42
Q

What is the oxidation state of Oxygen

A

-2

43
Q

What is the oxidation state F

A

-1

44
Q

What is oxidation in terms of a redox reaction?

A

Increase in oxidation state

45
Q

What is reduction in terms of a redox reaction?

A

Decrease in oxidation state

46
Q

What is an oxidizing agent and what is the reducing agent?

A

The oxidizing agent is the substance that causes the oxidation of another substance (it is always reduced)

The reducing agent causes the reduction in another substances ( it is always oxidized)

47
Q

What is the standard state of H2?

A

gas

48
Q

What is the standard state of N2?

A

gas

49
Q

What is the standard state of O2?

A

gas

50
Q

What is the standard state of F2?

A

gas

51
Q

What is the standard state of Cl2?

A

gas

52
Q

What is the standard state of CO?

A

gas

53
Q

What is the standard state of CO2?

A

gas

54
Q

What is the standard state of NO?

A

gas

55
Q

What is the standard state of noble gases

A

gas

56
Q

what is the standard state of H20

A

liquid

57
Q

What is the standard state of Br2

A

liquid

58
Q

What is the standard state of Hg

A

liquid

59
Q

What is the standard state of (Hg2)

A

liquid

60
Q

What is the standard state of I2

A

solid

61
Q

What is the standard state of metalloids

A

solid

62
Q

What is the standard state of other non-metals

A

solid

63
Q

Why is only the first H+ lost in H2SO4 a strong acid

A

When it becomes HSO4- and becomes H3O+ + SO4^2- it does not ionize completely in water

64
Q

what is boyles law and what is the formula

A

Pressure and volume are inversely related, as one decreases the other increases

P(1)V(1)=P(2)V(2)

65
Q

What is charles law and what is the formula

A

Volume and temperature are directly proportional, as one increases the other increases V(1)/T(1)=V(2)/T(2)

66
Q

What is Gay-Lussac’s Law

A

Pressure and temperature are directly proportional

P(1)/T1)=P(2)/T(2)

67
Q

What is Avogadro’s law

A

Moles and volume are directly proportional

V(1)/n(1)=V(2)/n(2)

68
Q

What is the standard pressure? What is the molar volume under standard conditions?

A

0.987 atm, 22.7 L

69
Q

what are the three postulates of kinetic molecular theory

A

the size of the particle is negligible (has no volume) even though they have mass.

the average kinetic energy of a particle is proportional to T (in K)

Collisions between particles or container walls are perfectly elastic (energy is transferred but not lost) (particles that collide do not exert any force on eachother

70
Q

what is the formulas for Kinetic Energy

A

KE=1/2mv^2, avgKE= 3/2RT

71
Q

how is molar mass expressed in root mean square

A

kg/L

72
Q

what is the R constant in the root mean square equation

A

8.3145 J/molxK

73
Q

what are the equations for density

A

d=mass/vol or d= PM/RT

74
Q

what does the kinetic molecular theory state

A

particles of different masses have the same average kinetic energy at a given temp

chem 400 (9 decks)

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