Worksheets2nd Semester (Nomenclature-Classifying Reactions-Percent Comp-Balancing-Moles-Gas Laws)
Total questions: 71
Worksheet time: 3hrs 46mins
Name
Class
Date
1.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
2.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
3.
Identify the phosphide ion
a)
P5+
b)
P3+
c)
P3-
d)
P4-
4.
What is the name for the NO3- ion?
a)
nitrate ion
b)
nitrite ion
c)
nitrogan ion
d)
nitride ion
5.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
6.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
7.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
8.
What is the metallic ion in the compound CuCl?
a)
Cu1+
b)
Cu2+
c)
Cu1-
d)
Cu2-
9.
What is the formula for aluminum sulfite?
a)
Al3S2
b)
AlSO4
c)
Al3(SO4)2
d)
Al2(SO3)3
10.
What is the formula for tin (II) chromate
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
11.
What is the formula for barium hydride?
a)
BaOH2
b)
Ba(OH)2
c)
BaH2
d)
BaOH
12.
Name the compound Mg3(PO4)2
a)
magnesium phosphate
b)
magnesium (III) phosphate
c)
magnesium phosphite
d)
magnesium phosphide
13.
Name the compound Fe(NO2)3
a)
iron nitrite
b)
iron (III) nitrate
c)
iron (III) nitrite
d)
ferric nitrite
14.
Name the compound NO3
a)
nitrogen trioxide
b)
nitrate
c)
nitrite
d)
dinitrogen pentoxide
15.
Name the compound CuO
a)
copper (II) oxide
b)
copper oxide
c)
copper (I) oxide
d)
carbon uranium oxide
16.
Name the compound SiCl4
a)
silicon tetrachloride
b)
sulfur tetrachloride
c)
silicon (IV) chloride
d)
silicon chloride
17.
If you have an oxyacid and it contains an -ite polyatomic ion, then acid's ending will change to _____.
a)
-ic
b)
-ous
c)
hydro-root-ic acid
d)
-ate
18.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
19.
bromic acid
a)
HBr
b)
H2Br
c)
HBrO3
d)
HBrO4
20.
Molecular compounds contain
a)
1 metal and 1 nonmetal
b)
only metals
c)
only nonmetals
d)
more than 2 elements (either metal or nonmetal)
21.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
22.
HI
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
23.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
24.
HF
a)
flouric acid
b)
hydrofluoric acid
c)
fluorate acid
d)
hydrogen fluoridic acid
25.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
26.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
27.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
28.
What is the molar mass of sodium?
a)
11
b)
23
c)
45.98
d)
3
29.
What is the molar mass of fluorine gas?
(beware!)
(beware!)
a)
18.998 g/mol
b)
38 g/mol
c)
9 g/mol
d)
18 g/mol
30.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
31.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
32.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
33.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
34.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
35.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
36.
We use the periodic table to calculate...
a)
mass
b)
molar mass
c)
moles
37.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
38.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
39.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
40.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
41.
Which has more molecules?
a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
42.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
43.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
44.
What is the percent by mass of calcium in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
45.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
46.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
47.
What is the empirical formula of the following molecular formula: C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
48.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
49.
What is the empirical formula for the following molecular formula: C5H12
a)
C5H12
b)
CH3
c)
CH2
d)
C2.5H6
50.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
51.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
52.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
53.
What is the mole ratio of H2O to H3PO4 in the following chemical equation? P4O10 + 6 H2O --> 4 H3PO4
a)
6:4
b)
4:6
c)
1:3
d)
3:1
54.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
55.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
221.378 g
b)
221 g
c)
220 g
56.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
57.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
58.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
1 Mg + 2 HCl --> 1 MgCl2 + 1 H2
1 Mg + 2 HCl --> 1 MgCl2 + 1 H2
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
59.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
60.
What is the correct formula for Boyle's Law?
a)
V1/T1=V2/T2
b)
P1V1=P2V2
c)
P1/T1=P2/T2
d)
PV=nRT
61.
Which variable is held constant when using Boyle's Law?
a)
Temperature
b)
Pressure
c)
Volume
d)
number of moles
62.
Which of the following temperatures is appropriate to convert 25oC into the Kelvin scale?
a)
373K
b)
272K
c)
372K
d)
273K
63.
What would you expect to see if temperature increased if you were using Charles's Law?
a)
volume would decrease proportionally
b)
volume would increase proportionally
c)
pressure would increase proportionally
d)
pressure would decrease proportionally
64.
What is the correct temperature on the Kelvin scale equal to 30oC?
a)
303K
b)
243K
c)
313K
d)
253K
65.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
66.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
67.
Boyle's law : The pressure and volume of a gas show a _____ relationship.
a)
Inverse
b)
Direct
68.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
69.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.
a)
0 K
b)
107 K
c)
207 K
d)
307 K
70.
Three gases, Ar, N2 and H2 are mixed in a sealed container. Ar has a pressure of 255 torr, N2 has a pressure of 228 torr and H2 has pressure of 752 torr. What is the total pressure in the container?
a)
483 torr
b)
270 torr
c)
1235 torr
71.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L.
a)
0.029 K
b)
0.021 K
c)
230 K
d)
34 K
100 %
