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Inorganic and Organic Chemistry > Mole Concept and Stoichiometry > Flashcards

Mole Concept and Stoichiometry Flashcards

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1
Q

basic unit/quantities

A

mole

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2
Q

of atom/element/compound

A

mole

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3
Q

avogadroโ€™s number

A

6.02x10^23

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4
Q

are non-zero digits and any zeroes contained between non-zero digits counted as significant figures

A

yes

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5
Q

how many significant figures in 300042

A

6 significant digits

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6
Q

are leading zeroes significant

A

no

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7
Q

how many significant figures in 0.0000034

A

2 significant figures

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8
Q

do trailing zeroes count if there is a decimal point

A

yes

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9
Q

how many significant figures in 0.0002500

A

4 significant digits

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10
Q

can trailing zeroes count if there is no decimal point

A

no

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11
Q

how many significant figures in 19000000

A

2

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12
Q

formula for molar mass

A

mass(g)/moles (mol)

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13
Q

illustrate the mole map

A

grade yourself accordingly

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14
Q

Determine the mass (g) of 2.50 moles of Na

A

57.5g (3 s.f.)

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15
Q

How many moles are present in 50.0g in MgCl2?

A

0.525 moles

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16
Q

How many Fe atoms are present in 10.0 moles of Fe

A

6.02๐‘ฅ10^24 ๐‘Ž๐‘ก๐‘œ๐‘š๐‘  ๐น๐‘’

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17
Q

Calculate the # of molecules present in 25.0g of CH3COOH (acetic acid)

A

2.51๐‘ฅ10^23 ๐‘š๐‘œ๐‘™๐‘’๐‘๐‘ข๐‘™๐‘’๐‘  ๐‘œ๐‘“ ๐ถ๐ป3๐ถ๐‘‚๐‘‚๐ป

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18
Q

Determine the # of Al atoms in 25.0 moles Al2S3

A

3.01๐‘ฅ10^25 ๐‘Ž๐‘ก๐‘œ๐‘š๐‘  ๐ด๐‘™

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19
Q

2 moles of Na is allowed to react with excess Cl2 to produce NaCl. Determine the # of moles of NaCl formed after the reaction

A

2 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐‘๐‘Ž๐ถ๐‘™

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20
Q

What mass (g) of Mg is needed to react with excess oxygen gas to produce 2.0 moles of MgO

A

48.608๐‘” ๐‘œ๐‘“ ๐‘€๐‘”

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21
Q

used to refer to extremely small particles such as atoms, molecules, and ions

A

mole

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22
Q

SI unit to denote the amount of substance

A

mole

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23
Q

amount of substance that contains as many elementary particles as in 0.12kg of carbon-12.

A

mole

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24
Q

experimentally determined value to describe a mole of a pure substance

A

6.02x10^23

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25
Q

honored using the Avogadroโ€™s number

A

Amadeo Avogadro

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26
Q

1 mole of any substance = ____particles

A

6.02x10^23

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27
Q

1 mol of Ag atom will contain ___ Ag atoms

A

6.02x10^23

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28
Q

born on August 9 1776 in Turin Piedmont-Sardinia (now part of Italy)

A

Lorenzo Romano Amadeo Carlo Avogadro

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29
Q

father of Avogadro (lawyer), well-known magistrate and senator in Piedmnt region of northern Italy

A

Fillippo Avogadro

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30
Q

Avogadroโ€™s mother, a noblewoman

A

Anna Vercellone of biella

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31
Q

Avogadro received his doctorate in ecclesiastical law

A

age of 20

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32
Q

Three different types of molecules that Avogadro described

A

integral molecule
constituent molecule
elementary molecule

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33
Q

when did Avogadro stated that โ€œequal volumes of all gases at the same temperature and pressure contain the same number of moleculesโ€

A

1811

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34
Q

was given as equivalent to 1/12 the mass of carbon-12 and that all other atomic masses of the elements are determined relative to carbon 12

A

atomic mass (amu)

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35
Q

as such as the mass in grams of one mole of any substance is called with the unit of grams/mole

A

molar mass

36
Q

Determine the molar mass of the following compounds:

A. MgO

A

40.303 g/mol

37
Q

Determine the molar mass of the following compounds:

H2SO4

A

98.5206 g/mol

38
Q

Determine the molar mass of the following compounds:

Zn3(PO4)2

A

=386.08 ๐‘”/๐‘š๐‘œ๐‘™

39
Q

Francium, the alkali metal named after France, was discovered by Marguerite Perey in 1939. Though known to be radioactive, as of today it has no known uses because it is unstable and rare. Determine the number of atoms present in 2.50 moles of Francium, Fr.

A

1.505525๐‘ฅ1024 ๐‘Ž๐‘ก๐‘œ๐‘š๐‘  ๐‘œ๐‘“ ๐น๐‘Ÿ

40
Q

Lithium is an element that produces a red flame. Calculate the number of moles in Li in 7.35x1024 atoms of Li

A

12.20504475 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐‘œ๐‘“ ๐ฟ๐‘–

41
Q

Incomplete combustion of fuels produce carbon monoxide, a colorless, tasteless, odorless poisonous gas. Calculate the number of CO molecules present in 4.50 moles of CO.

A

2.709945๐‘ฅ1024 ๐‘š๐‘œ๐‘™๐‘’๐‘๐‘ข๐‘™๐‘’๐‘  ๐ถ๐‘‚

42
Q

Convert 5.78x1022 molecules released in the atmosphere in number of moles

A

0.09597980771 ๐ถ๐‘‚ ๐‘š๐‘œ๐‘™๐‘’๐‘๐‘ข๐‘™๐‘’๐‘ 

43
Q

determines the number of moles present for every mole of the compound

A

subscript

44
Q

Nitrous oxide with the molecular formula N2O is also known as laughing gas. It is colorless and odorless and is known to have analgesic and anesthetic purposes

Calculate the mass (g) of 8.75 moles N2O

A

385.09625 ๐‘” ๐‘2๐‘‚

45
Q

Nitrous oxide with the molecular formula N2O is also known as laughing gas. It is colorless and odorless and is known to have analgesic and anesthetic purposes

If the mass of N2O is 35.89g, what is the corresponding number of moles?

A

0.8154 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐‘2๐‘‚

46
Q

Hydrogen cyanide, HCN, also known as prussic acid is a toxic compound that boils above 26oC. It can readily be absorbed through inhalation, ingestion, or even by dermal exposure.

Calculate the number of moles of H atom present in 2.50 moles of HCN

A

2.50 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐ป

47
Q

Determine the number of N atom present in 1.25g of HCN

A

2.784685525๐‘ฅ1022 ๐‘Ž๐‘ก๐‘œ๐‘š๐‘ 

48
Q

Compute the mass in grams of H and N atoms present in 5.85 moles of HCN

A

81.90351 ๐‘” ๐‘

49
Q

used as a safety device in most vehicles

A

air bags

50
Q

occurs that allow the air bag to inflate and provide protection during collision

A

chemical reactions

51
Q

its decomposition to sodium metal and nitrogen gas is the main chemical reaction involved

A

sodium azide

52
Q

also incorporated in air bags to ensure that the bag is inflated enough

A

oxidizers

53
Q

ordinary airbag has what volume

A

36 liters

54
Q

hwow many sodium azide must be decomposed to produce the volume of 36 liters of nitrogen gas

A

130g sodium azide

55
Q

science of measuring the quantitative proportions or mass ratios in which chemical elements stand to one another

A

stoichiometry

56
Q

Stoicheion means

A

element

57
Q

metron means

A

measure

58
Q

involves the mass relationships between reactants and products in a chemical reaction

A

stoichiometry

59
Q

all reaction stoichiometry relationships start here

A

balanced chemical equation

60
Q

gives the relative numbers of moles of reactants and products

A

equation

61
Q

is used to solve problems from the balanced equations

A

ratios

62
Q

N2 + 3H2 -> 2NH3

how many are the following:

Number of atoms: ___ atoms of Nitrogen, _ atoms of Hydrogen, and _ atoms of ammonia

A

Number of atoms: 2 atoms of Nitrogen, 6 atoms of Hydrogen, and 8 atoms of ammonia

63
Q

N2 + 3H2 -> 2NH3

how many are the following:

Number of molecules: _ molecule of Nitrogen, _ molecules of hydrogen, and _ molecules of ammoni

A

Number of molecules: 1 molecule of Nitrogen, 3 molecules of hydrogen, and 2 molecules of ammoni

64
Q

N2 + 3H2 -> 2NH3

how many are the following:

Number of relative moles: _ mole of nitrogen, _ relative
moles of hydrogen, _ relative moles of ammonia

A

Number of relative moles: 1 mole of nitrogen, 3 relative
moles of hydrogen, 2 relative moles of ammonia

65
Q

N2 + 3H2 -> 2NH3

how many are the following:

Mass:
of Nitrogen,
of Hydrogen,
of ammonium

A

Mass: 28.012g of Nitrogen, 6.0468g of Hydrogen, 34.0588g of ammonium

66
Q

N2 + 3H2 -> 2NH3

how many are the following:

volume:
of Nitrogen,
of Hydrogen,
of ammonium

A

Volume: 22.4L of nitrogen, 67.2L of hydrogen, and 44.8L of ammonia

67
Q

Magnesium metal can react with dry ice (solid CO2) to produce magnesium oxide and carbon. The chemical reaction is shown below

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2 (๐‘ )โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

Balance the chemical equation

A

2๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2 (๐‘ )โ†’2๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

68
Q

Magnesium metal can react with dry ice (solid CO2) to produce magnesium oxide and carbon. The chemical reaction is shown below

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2 (๐‘ )โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

Determine the number of moles carbon produced when 5.0 mole of Mg is used

A

=2.50 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐ถ

69
Q

Magnesium metal can react with dry ice (solid CO2) to produce magnesium oxide and carbon. The chemical reaction is shown below

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2 (๐‘ )โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

c. If 10.0 moles of MgO must be obtained, how much CO2 is needed

A

5.0 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐ถ๐‘‚2

70
Q

Magnesium metal can react with dry ice (solid CO2) to produce magnesium oxide and carbon. The chemical reaction is shown below

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2 (๐‘ )โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

If the amount of Mg in letter b is totally consumed, how much CO2 is required

A

2.50 ๐‘š๐‘œ๐‘™๐‘’๐‘  ๐ถ๐‘‚2

71
Q

is an effective cleaning agent commonly found in households. It contains sodium hypochlorite, NaClO, which can produce toxic chlorine gas, Cl2, when combined with muriatic acid (HCl).

A

bleach

72
Q

๐ป๐‘‚๐ถ๐‘™+๐ป๐ถ๐‘™โ†’๐ป2๐‘‚+๐ถ๐‘™2

Determine the number of moles of Cl2 produced from 15.0g HOCl

A

0.286 ๐‘š๐‘œ๐‘™๐‘’ ๐ถ๐‘™2

73
Q

๐ป๐‘‚๐ถ๐‘™+๐ป๐ถ๐‘™โ†’๐ป2๐‘‚+๐ถ๐‘™2

What mass (g) of HCl is needed to completely react with 4.50 moles HOCl

A

164.0421๐‘” ๐ป๐ถ๐‘™

74
Q

is the starting material that is totally consumed when the chemical reaction is completed

A

limiting reagent or reactant

75
Q

It limits the amount of product that is formed in a chemical reaction

A

limiting reagent

76
Q

In most cases, problems dealing with limiting reagents give the amount (mass or moles) of both reactants

A

limiting reagent

77
Q

How many moles of water can we make from 6 moles of hydrogen and 4 moles of oxygen?

2 ๐ป2 (๐‘”)+ ๐‘‚2(๐‘”)โ†’2๐ป2๐‘‚(๐‘”)

A

limiting reagent = H2
Amount of H2O = 6 moles

78
Q

What mass of iron in grams could be formed from 113g Al and 279g Fe2O3

2 ๐ด๐‘™ (๐‘ )+ ๐น๐‘’2๐‘‚3 (๐‘ )โ†’ ๐ด๐‘™2๐‘‚3 (๐‘ )+2 ๐น๐‘’ (๐‘™)

A

limiting reactant Fe2O3
amount of Fe = 195g

79
Q

What mass of C3H3N in grams can be made when 21.6g of C3H6 react with 21.6g of NO

4๐ถ3๐ป6(๐‘”)+6 ๐‘๐‘‚(๐‘”)โ†’4๐ถ3๐ป3๐‘(๐‘ )+6๐ป2๐‘‚(๐‘™)+๐‘2(๐‘”)

A

25.5๐‘” ๐ถ3๐ป3๐‘
limiting reagent 21.6g

80
Q

Consider the reaction between magnesium and carbon dioxide:

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

If 4.50g each of Mg and CO2 were reacted, how many grams of carbon will be produced?

A

limiting reagent = Mg
carbon produced = 1.11g C

81
Q

Consider the reaction between magnesium and carbon dioxide:

๐‘€๐‘” (๐‘ )+๐ถ๐‘‚2โ†’๐‘€๐‘”๐‘‚ (๐‘ )+๐ถ (๐‘ )

How much of the excess reagent will be left after the reaction?

A

0.43๐‘” ๐ถ๐‘‚2

82
Q

ratio of actual yield/theoretical yield

A

percent yield

83
Q

formula of percent yield

A

actual yield/theoretical yield x 100

84
Q

amount of product made under ideal conditions, the most possible product you can make (almost never happens), the number you calculate using stoichiometry

A

theoretical yield

85
Q

amount of product made during the actual reaction in the laboratory

A

actual yield

86
Q

If the amount of carbon obtained in sample exercise 2.2 is 1.00g, determine the percentage yield of the reaction

theoretical yield = 1.11g

A

90.1%

Inorganic and Organic Chemistry (19 decks)

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