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Percent
Composition
Empirical
and
Molecular
Formulas
Vocabulary
The Mole
Avogadro’s
Number
Gram
atomic
weight
100
100
100
100
100
100
200
200
200
200
200
200
300
300
300
300
300
300
400
400
400
400
400
400
500
500
500
500
500
500
Define average atomic mass
A 100
Weighted average of all the
isotopes of an element
A 100
Define mass percent
A 200
Percent by mass of a
particular component of a
compound or mixture
A 200
Define molar mass
A 300
Mass of one mole of a
substance
A 300
Define empirical formula
A 400
Simplest whole number ratio
of atoms in a compound
A 400
Define molecular formula
A 500
Actual number of atoms of
each element in a molecule
A 500
A 14.8-g sample of magnesium
represents how many moles?
B 100
0.608 mol Mg
B 100
A 9.24-g sample of sodium
represents how many moles?
B 200
0.402 mol Na
B 200
Convert 48 g O2 to mol O2.
B 300
1.5 mol O2
B 300
Convert:
3.0 x 1024 molecules H2O =
______________ mol H2O
B 400
5.0 mol H2O
B 400
A 14.2-g sample of Ba(NO3)2
contains how many moles of
Ba(NO3)2?
B 500
0.0543 mol Ba(NO3)2
B 500
How many atoms of calcium are
present in 80.0 g of calcium?
C 100
1.20 x 1024 atoms Ca
C 100
How many atoms are there in
58.7 g of nickel?
C 200
6.02 x 1023 atoms Ni
C 200
How many molecules of O2 are
there in 4.0 mol of O2?
C 300
2.4 x 1024 molecules O2
C 300
DAILY
Place A Wager
DOUBLE
C 400
6.00 g of water contains how
many molecules of water?
C 400
2.10 x 1023 molecules H2O
C 400
A mole of sulfur trioxide
molecules contains how many
oxygen atoms? (Round to four
significant figures)
C 500
1.807 x 1024 oxygen atoms
C 500
Calculate the mass of 20.0 moles
of He.
D 100
80.1 g He
D 100
Calculate the mass of 8.43 x 1026
atoms of silver.
D 200
1.51 x 105 g Ag
D 200
Calculate the mass of 3.50 mol
of sulfur dioxide.
D 300
224 g SO2
D 300
What is the mass of 2.00
moles of Ca(OH)2?
D 400
148.2 g Ca(OH)2
D 400
Calculate the mass of sulfur in
2.0 mol of H2SO4.
D 500
64 g H2SO4
D 500
The mass percent of oxygen in
CaO is
E 100
28.5 % O in CaO
E 100
What is the percent (by mass) of
carbon in glucose, C6H12O6?
E 200
40.0 % C in C6H12O6
E 200
The mass percent of nitrogen in
NH4Cl is
E 300
26.2 % N in NH4Cl
E 300
Determine the percentage
composition (by mass) of all the
elements in H2SO4.
E 400
2.06 % H
32.69 % S
65.25 % O
E 400
Determine the percentage
composition (by mass) of each of
the elements in NH4NO3.
E 500
35.00 % N
59.96 % O
5.04 % H
E 500
Which of the following has the
empirical formula CH2?
a. C2H6
b. H2CO3
c. C6H6
d. C6H12
e. C2H4O
F 100
d. C6H12
F 100
Calculate the empirical
formula of a compound that is
85.6% C and 14.4% H (by
mass).
F 200
CH2
F 200
A 7.33-g sample of
lanthanum, La, combines
with oxygen to give 10.29 g
of the oxide. Calculate the
empirical formula of this
oxide.
F 300
La2O7
F 300
Calculate the molecular formula
of a compound with the
empirical formula CH2O and a
molar mass of 150 g/mol.
F 400
C5H10O5
F 400
The empirical formula for
acetic acid is CH2O. Its molar
mass is 60 g/mol. The
molecular formula is
F 500
C2H4O2
F 500
The Final Jeopardy Category is:
Using mole to mole ratios to
solve for individual parts of a
compound
Please record your wager.
Click on screen to begin
How many grams of nitrogen are
there in 23.8 g of ammonia, NH3?
Click on screen to continue
23.8 g NH3 x
1
1 mole N
1 mole NH3
1 mole NH3
17.034 g NH3
x
14.01 g N
1 mole N
= 19.6 g N
Click on screen to continue
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