Page 1 of 35
CHEM103 / CHEM 103 MODULES 4 - 6 & FINAL EXAMS:
(LATEST UPDATES STUDY BUNDLE
PACKAGE) GENERAL CHEMISTRY I WITH LAB |
QUESTIONS & ANSWERS | GRADE A | 100%
CORRECT - PORTAGE LEARNING
Avogadro's number .....ANSWER.....6.022 x 10^23 atoms = 1
mole
1 u = ___ g .....ANSWER.....1.661 x 10 ^-24 g
formula mass .....ANSWER.....the sum of the average atomic
masses of each atom represented in the chemical formula and is
expressed in atomic mass units.
--The formula mass of a covalent compound is also called the
molecular mass.
The chemical identity of a substance is defined by
.....ANSWER.....the types and relative numbers of atoms
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composing its fundamental entities (molecules in the case of
covalent compounds, ions in the case of ionic compounds).
A compound's percent composition provides .....ANSWER.....the
mass percentage of each element in the compound.
calculate the formula mass of a substance by
.....ANSWER.....summing the average atomic masses of all the
atoms represented in the substance's formula.
A mole is defined as .....ANSWER.....the amount of substance
containing the same number of discrete entities (such as atoms,
molecules, and ions) as the number of atoms in a sample of pure
12-C weighing exactly 12 g
percent composition .....ANSWER.....the percentage by mass of
each element in a compound
i.e. mass X / mass compound x 100%
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stoichiometry .....ANSWER.....refers to the quantitative
relationships between amounts of reactants and products in a
chemical reaction.
Combustion .....ANSWER.....a reaction in which an element or
compound burns in air or oxygen
--The combustion of compounds containing hydrogen and carbon
(CxHy) will always produce two products: water (H2O) and
carbon dioxide (CO2).
--The same is true for the combustion of compounds containing
hydrogen, carbon and oxygen (CxHyOz)
Chemical formulas provide the .....ANSWER.....identities of the
reactants and products involved in the chemical change, allowing
classification of the reaction
Coefficients provide the .....ANSWER.....relative numbers of these
chemical species, allowing a quantitative assessment of the
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relationships between the amounts of substances consumed and
produced by the reaction.
stoichiometric factor .....ANSWER.....ratio of coefficients in a
balanced chemical equation, used in computations relating
amounts of reactants and products
Limiting Reactant .....ANSWER.....A reactant that is totally
consumed during a chemical reaction, limits the extent of the
reaction, and determines the amount of product.
theoretical yield .....ANSWER.....The amount of product that may
be produced by a reaction under specified conditions, as
calculated per the stoichiometry of an appropriate balanced
chemical equation, is called the theoretical yield of the reaction
actual yield .....ANSWER.....the amount of product that forms
when a reaction is carried out in the laboratory
percent yield .....ANSWER.....actual yield/theoretical yield x 100
CHEM103 / CHEM 103 MODULES 4 - 6 & FINAL EXAMS:
(LATEST UPDATES STUDY BUNDLE
PACKAGE) GENERAL CHEMISTRY I WITH LAB |
QUESTIONS & ANSWERS | GRADE A | 100%
CORRECT - PORTAGE LEARNING
Avogadro's number .....ANSWER.....6.022 x 10^23 atoms = 1
mole
1 u = ___ g .....ANSWER.....1.661 x 10 ^-24 g
formula mass .....ANSWER.....the sum of the average atomic
masses of each atom represented in the chemical formula and is
expressed in atomic mass units.
--The formula mass of a covalent compound is also called the
molecular mass.
The chemical identity of a substance is defined by
.....ANSWER.....the types and relative numbers of atoms
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composing its fundamental entities (molecules in the case of
covalent compounds, ions in the case of ionic compounds).
A compound's percent composition provides .....ANSWER.....the
mass percentage of each element in the compound.
calculate the formula mass of a substance by
.....ANSWER.....summing the average atomic masses of all the
atoms represented in the substance's formula.
A mole is defined as .....ANSWER.....the amount of substance
containing the same number of discrete entities (such as atoms,
molecules, and ions) as the number of atoms in a sample of pure
12-C weighing exactly 12 g
percent composition .....ANSWER.....the percentage by mass of
each element in a compound
i.e. mass X / mass compound x 100%
,Page 3 of 35
stoichiometry .....ANSWER.....refers to the quantitative
relationships between amounts of reactants and products in a
chemical reaction.
Combustion .....ANSWER.....a reaction in which an element or
compound burns in air or oxygen
--The combustion of compounds containing hydrogen and carbon
(CxHy) will always produce two products: water (H2O) and
carbon dioxide (CO2).
--The same is true for the combustion of compounds containing
hydrogen, carbon and oxygen (CxHyOz)
Chemical formulas provide the .....ANSWER.....identities of the
reactants and products involved in the chemical change, allowing
classification of the reaction
Coefficients provide the .....ANSWER.....relative numbers of these
chemical species, allowing a quantitative assessment of the
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relationships between the amounts of substances consumed and
produced by the reaction.
stoichiometric factor .....ANSWER.....ratio of coefficients in a
balanced chemical equation, used in computations relating
amounts of reactants and products
Limiting Reactant .....ANSWER.....A reactant that is totally
consumed during a chemical reaction, limits the extent of the
reaction, and determines the amount of product.
theoretical yield .....ANSWER.....The amount of product that may
be produced by a reaction under specified conditions, as
calculated per the stoichiometry of an appropriate balanced
chemical equation, is called the theoretical yield of the reaction
actual yield .....ANSWER.....the amount of product that forms
when a reaction is carried out in the laboratory
percent yield .....ANSWER.....actual yield/theoretical yield x 100
