Portage Chemistry 103 Module 2 Exam Study
2.1: MOLECULAR WEIGHT Correct Answer: A compound is made up of two or more elements combined in a definite ratio that is represented by a molecular formula. Each of these elements has a certain atomic weight, which can be found in the periodic table. Th...
Portage Chemistry 103 Module 2 Exam Study
2.1: MOLECULAR WEIGHT Correct Answer: A compound is made up of two or more elements combined
in a definite ratio that is represented by a molecular formula. Each of these elements has a certain
atomic weight, which can be found in the periodic table. The sum of the atomic weights of the atoms in
the molecular formula is called the formula weight or molecular weight or formula mass.
Ca3(PO4)2 Correct Answer: calcium phosphate
Molecular Weight =
3 Ca= 3 x 40.08=120.24
2 P=2 x 30.97=61.94
8 O=8 x 16.00=128.00
Total 310.18
2.2: MOLES Correct Answer: Chemical compounds react with one another in amounts that are based on
their molecular weights; this chemically reactive amount of compound is called a mole.
moles Correct Answer: = grams / molecular weight
Calculate the number of moles in 10.0 grams of each of the following compounds: Correct Answer:
Ca3(PO4)2 10.0 g ÷ 310.18 = 0.0322 mol (3 sig fig because of 10.0 g)
C3H5O2Cl 10.0 g ÷ 108.52 = 0.0921 mol
Al2(SO4)3 10.0 g ÷ 342.17 = 0.0292 mol
Ca3(PO4)2 0.0500 mol x 310.18 = 15.5 g
C3H5O2Cl 0.0500 mol x 108.52 = 5.43 g
Al2(SO4)3 0.0500 mol x 342.17 = 17.1 g
2.3: PERCENT COMPOSITION Correct Answer: he molecular formula represents the definite ratio of
elements in a compound. The weight of each element present in the compound represents a certain
percentage of the total weight of the compound. The percentage of each element present in a
compound is called the % composition of the compound.
The percentage of an element present in a compound can be calculated as shown below: Correct
Answer: % of an element = weight of element / molecular weight of compound x 100
Ca3(PO4)2 Correct Answer: 3 Ca = 3 x 40.08= 120.24
2 P = 2 x 30.97= 61.94
8 O = 8 x 16.00 = 128.00
310.18
% Ca = (120.24 ÷ 310.18) x 100 = 38.76%
%P = (61.94 ÷ 310.18) x 100 = 19.97%
, %O = (128.00 ÷ 310.18) x 100 = 41.27%
2.4: EMPIRICAL FORMULA Correct Answer: If the formula of a compound is known, the % composition
of the compound can be determined. This process can be done in reverse: The formula of the compound
can be determined if the % of each element present in the compound is known. The formula calculated
from % composition is known as the empirical formula (or the simplest formula). The actual molecular
formula is some multiple of this simplest formula, which is determined by knowing the molecular
weight.
To determine the empirical formula: Correct Answer: (1) Divide each element % by its exact atomic
weight to give a set of numbers.
(2) Divide the smallest of this set of decimal numbers into each of the numbers (including itself) to yield
a second set of numbers.
(3a) Round off each of the second set of decimal numbers to a whole number.
OR
(3b) If the numbers derived from the division in step 2 are recognized as exact decimal equivalents of
fractions (such as n.25 = 1/4, n.333 = 1/3, n.5 = 1/2, n.666 = 2/3, n.75 = 3/4), multiply all of the numbers
derived by division by the denominator of the recognized fraction to give whole numbers.
(4) Each whole number is the number of atoms of that element in the empirical formula.
% Composition of a compound is: Correct Answer: 32.37% Na; 32.37% Na ÷ 22.99 = 1.408
22.58%S; 22.58% S ÷ 32.07 = 0.704 (smallest number of the set)
45.05% O; 45.05% O ÷ 16.00 = 2.816
0.704 is the smallest of this set of numbers, so it is divided into each of the set of numbers.
Na = 1.408 ÷ 0.704 = 2 Na
S = 0.704 ÷ 0.704 = 1 S
O = 2.816 ÷ 0.704 = 4 O
Na2SO4
2.5: BALANCING CHEMICAL EQUATIONS Correct Answer: When certain chemical materials are added to
one another, they undergo a chemical reaction in which the atoms of the materials separate from one
another and recombine in a new way to form new materials. This chemical reaction can be described by
a chemical reaction equation in which the reactants (starting materials) are written on the left side of
the equation and the products (final materials) are written on the right side of the equation, separated
by an arrow which points from left to right (some sites use an equals sign here but this is incorrect
because the only thing equal about this equation is the number of atoms, once balanced), an example of
which is shown below:
NaOH + HCl → NaCl + H2O
The reaction equation is read as follows:
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