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WorksheetsChemistry Spring 2025 Final Question Pool
Total questions: 101
Worksheet time: 51mins
Name
Class
Date
1.
Identify any incorrect names.
a)
Calcium (II) oxide
b)
Aluminum oxide
c)
Ammonium peroxide
d)
Monosulfur dioxide
e)
Tetraiodide nonoxide
2.
Identify formulas that are written incorrectly.
a)
Na2(C2O4)
b)
Mg(NH4)2
c)
SnCr2O7
d)
CaCO3
e)
AlCl3
3.
What makes a compound an acid?
a)
When the compound is dissolved in water, it produces hydrogen ions.
b)
When the compound is dissolved in water, it produces hydroxide ions.
c)
It is soluble in water.
d)
When the compound is dissolved in water, it produces an equal number of hydrogen and hydroxide ions.
4.
What makes a compound a base?
a)
When the compound is dissolved in water, it produces hydrogen ions.
b)
When the compound is dissolved in water, it produces hydroxide ions.
c)
It is soluble in water.
d)
When the compound is dissolved in water, it produces an equal number of hydrogen and hydroxide ions.
5.
Two compounds that contain copper and chlorine have the following masses:
Compound A: 32.10 g of Cu and 17.90 g of Cl
Compound B: 23.64 g of Cu and 26.37 g of Cl.
Are the compounds the same (meaning both would have the same chemical formula)? If not, what is the lowest whole-number mass ratio of copper that combines with a given mass of chlorine?
a)
Yes, they are the same compounds.
b)
No, they are not; it is a rough 2:1 ratio.
c)
No, they are not; it is a rough 1:2 ratio.
d)
No, they are not; it is a rough 8:5 ratio.
6.
Nitrous oxide, known as laughing gas, is used as an anesthetic in dentistry. The mass ratio of nitrogen to oxygen is 7:4 for nitrous oxide. A 68-gram sample of a compound composed of nitrogen and oxygen contains 42 g of nitrogen. Is the sample nitrous oxide?
a)
No, the sample's ratio of nitrogen to oxygen is 21:13.
b)
No, the sample's ratio of nitrogen to oxygen is 13:26.
c)
Yes, the sample's ratio of nitrogen to oxygen is 7:4.
d)
Yes, the sample's ratio of nitrogen to oxygen is 4:7.
7.
Name BaO
(a)
8.
Name NCl3
(a)
9.
Name HClO3
(a)
10.
Name SO2
(a)
11.
Name Fe(OH)3
(a)
12.
Name PbCrO4
(a)
13.
Name HCN
(a)
14.
Strontium oxide
a)
SrO
b)
Sr2O
c)
SrO2
d)
Sr2O2
15.
Boron trichloride
a)
BCl3
b)
BCl2
c)
B3Cl
d)
BCl4
16.
Nitrogen monoxide
a)
NO
b)
N2O
c)
NO2
d)
N3O5
17.
Dicarbon pentoxide
a)
C2O5
b)
CO5
c)
C2O
d)
CO
18.
Hydroselenic acid
a)
H2Se
b)
HSe
c)
H3Se
d)
H2S
19.
Cobalt(II) hydroxide
a)
Co(OH)2
b)
CoOH
c)
Co2OH
d)
CoOH2
20.
Hydrosulfuric acid
a)
H2S
b)
H2SO4
c)
H2SO3
d)
HS
21.
How many phosphorus atoms are in a representative particle of (NH4 )2 HPO4 ?
a)
9
b)
3
c)
1
d)
4
22.
What is the molar mass of atomic fluorine?
a)
18.998 grams
b)
9 grams
c)
2.111 grams
d)
170.982 grams
23.
What is the molar mass of silicon dioxide?
a)
60.083 g/mol
b)
44.084 g/mol
c)
72.169 g/mol
d)
88.168 g/mol
24.
How many moles of NaCl is 2.41 x 10^23 formula units of NaCl?
a)
4.0 mol NaCl
b)
0.40 mol NaCl
c)
0.25 mol NaCl
25.
About many moles of oxygen gas, O2, is 1.776 grams of oxygen gas?
a)
9 mol
b)
18 mol
c)
0.111 mol
d)
0.056 mol
26.
Which of the following contains the most molecules?
a)
1 mol H2O2
b)
1 mol C2H6
c)
1 mol CO
d)
They have the same number of molecules.
27.
How many moles of SO2 are present in 0.23 kg of SO2?
a)
3.6 mol SO2
b)
3.6 x 10^-3 mol SO2
c)
4.8 mol SO2
d)
4.8 x 10^-3 mol SO2
28.
How many grams are present in 5.66 mol of CaCO3?
a)
566.49 g CaCO3
b)
0.06 g CaCO3
c)
17.68 g CaCO3
d)
385.38 g CaCO3
29.
Find the number of moles in 508 grams of ethanol (C2H6O).
a)
11.03 mol C2H6O
b)
23403.05 mol C2H6O
c)
17.51 mol C2H6O
d)
14741.144 mol C2H6O
30.
A gas has a density of 0.902 g/L at STP. What is the molar mass of the gas?
a)
20.2 g/mol
b)
0.04 g/mol
c)
24.8 g/mol
d)
23.3 g/mol
31.
Three balloons are filled with three different gaseous compounds. The balloons each have a volume of 22.4 L at STP. Do the balloons have the same mass or contain the same number of molecules?
a)
Same mass
b)
Same number of molecules
c)
Same mass and same number of molecules
d)
Different mass and different number of molecules
32.
What information can you use to calculate the empirical formula of a compound, knowing nothing else?
a)
Use the percent composition of the compound
b)
Use the molar mass of the compound
c)
Use the molar volume of the compound
d)
Use the empirical formula of the compound
33.
Determine the percent composition of a the compound that forms when 222.6 g N combines completely with 77.4 g O.
a)
74.2% N; 25.8% O
b)
25.8% N; 74.2% O
c)
34.77% N; 65.23% O
d)
65.23% N; 34.77% O
34.
How much calcium is in calcium acetate? (That is, what is the percent composition of calcium acetate, Ca(C2H3O2)2? Then, tell me the percentage for calcium.)
a)
25.3%
b)
7.6%
c)
3.8%
d)
25.4%
e)
6.4%
35.
How many grams of hydrogen are in 150 grams of hydrochloric acid (HCl)?
a)
4.15 g H
b)
5424.3 g H
c)
4.27 g H
d)
4.20 g H
36.
Which of the following molecular formulas are also empirical formulas?
a)
C5H10O5
b)
C6H12O2
c)
C55H72MgN4O5
d)
C12H17ON
37.
Which of the following contains the largest number of atoms?
a)
82.0 g Kr
b)
0.842 mol C2H4
c)
36.0 g N2
d)
1 mol H2O
38.
How do we indicate in a chemical equation that we need heat?
a)
Double arrow
b)
Put a delta over the arrow
c)
Put a thermometer over the arrow
d)
Put the symbol of the heat source over the arrow
39.
Which law do you need to keep in mind as you balance a chemical equation?
a)
Law of conservation of mass
b)
Law of conservation of energy
c)
Law of conservation of momentum
d)
Law of special relativity
40.
If you see (aq) next to a reactant or product in a chemical equation, what does that mean?
a)
The substance is dissolved in water.
b)
The substance is dissolved in oil.
c)
The substance is a liquid.
d)
Water is dissolved in the substance.
41.
Identify 5 general types of reactions.
a)
Combination (Synthesis)
b)
Decomposition
c)
Single-replacement
d)
Double-replacement
e)
Combustion
42.
For the neutralization reaction of sodium hydroxide and hydrobromic acid, water and the salt ___________ are produced.
a)
sodium bromide
b)
sodium bromate
c)
bromine hydroxide
d)
sodium bromite
43.
Classify the following chemical equation: Ca + 2HCl ---> CaCl2 + H2
a)
Combination (Synthesis)
b)
Decomposition
c)
Single-replacement
d)
Double-replacement
e)
Combustion
44.
What should the coefficient of oxygen gas (O2) be for the complete combustion equation of vanillin (C8H8O3)?
(a)
45.
What is a net ionic equation?
a)
It is a chemical equation that shows only the particles involved in the reaction and is balanced with respect to both mass and charge.
b)
It is chemical equation.
c)
It is a chemical equation that shows only the particles not involved in the reaction and is balanced with respect to both mass and charge.
d)
It is a chemical equation that deals with ionic compounds.
46.
According to our solubility rules for ionic compounds table, will sodium carbonate dissolve in water?
a)
Yes
b)
No
47.
Which of the following is the balanced net ionic equation for Pb(NO3)2 (aq) +H2SO4 (aq) --> PbSO4 (s) + HNO3 (aq)?
a)
[Pb]2+ (aq) + [SO4]2- (aq) --> PbSO4 (s)
b)
[NO3]- (aq) + [H]+ (aq) --> HNO3 (aq)
c)
2 [Pb]2+ (aq) + 2 [SO4]2- (aq) --> 2 PbSO4 (s)
d)
[NO3]- (aq) + [H]+ (aq) --> HNO3 (s)
48.
What is the name of the precipitate that is formed when solutions of Ca(NO3)2 and Na2CO3 are mixed?
(a)
49.
Identify the spectator ions for the following reaction.
Na3PO4 (aq) + FeCl3 (aq) --> NaCl (aq) + FePO4 (s)
a)
Na+
b)
Fe3+
c)
[PO4]3-
d)
Cl-
50.
After balancing the chemical equation: SO2 (g) + O2 (g) --> SO3 (g), the correct coefficient of sulfur dioxide is (a) .
51.
After balancing the chemical equation: SO2 (g) + O2 (g) --> SO3 (g), the correct coefficient of oxygen gas is (a) .
52.
After balancing the chemical equation: SO2 (g) + O2 (g) --> SO3 (g), the correct coefficient of sulfur trioxide is (a) .
53.
After balancing the chemical equation: Zn + H2SO4 --> ZnSO4 + H2, the coefficient of zinc is (a) .
54.
After balancing the chemical equation: Zn + H2SO4 --> ZnSO4 + H2, the coefficient of sulfuric acid is (a) .
55.
After balancing the chemical equation: Zn + H2SO4 --> ZnSO4 + H2, the coefficient of zinc sulfate is (a) .
56.
After balancing the chemical equation: Zn + H2SO4 --> ZnSO4 + H2, the coefficient of hydrogen gas is (a) .
57.
Identify the quantities that are always conserved in chemical reaction.
a)
Atoms
b)
Mass
c)
Volume
d)
Ions
e)
Color
58.
Which of the following methods does NOT prove that a chemical equation is balanced (i.e. it obeys the law of conservation of mass)?
a)
Show that the number of atoms of each element are the same on the reactant and product sides.
b)
Show that the total net charges are the same on the reactant and product sides.
c)
Show that if you take the molar masses of each compound multiplied by its coefficient, then the total mass of the reactants will be the same as the total mass of the products.
59.
According to the following chemical equation, you need at least __________ molecules of hydrogen gas to form 2 moles of water vapor.
2 H2 (g) + O2 (g) --> 2 H2O
a)
2
b)
1.2044 x 10^24
c)
2.016
d)
1.2140 x 10^24
e)
1.1948 x 10^24
60.
What do we call the conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles?
a)
Mole ratio
b)
Mole fraction
c)
Mole conversion
d)
Coefficient ratio
61.
Why is a balanced chemical equation essential for stoichiometric calculations?
a)
You need it to get your mole ratios.
b)
You need it to get substances' formulas.
c)
You need it to get substances' molar masses.
d)
You need it to get substances molar volumes at STP.
62.
A reagent that determines how much product can be formed in a reaction is called a(n)
a)
limiting reagent.
b)
excess reagent.
c)
stopping reagent.
d)
surplus reagent.
63.
A reactant that is not completely used up in a reaction is called a(n)
a)
limiting reagent.
b)
excess reagent.
c)
stopping reagent.
d)
surplus reagent.
64.
How many moles of ammonia are required to fully react 120 grams of fluorine gas?
5 F2 (g) + 2 NH3 (g) --> N2F4 (g) + 6 HF(g)
a)
1.26 mol NH3
b)
7.90 mol NH3
c)
2.53 mol NH3
d)
21.52 mol NH3
65.
How many liters of hydrogen fluoride gas are produced if 2 mol of dinitrogen tetrafluoride gas were produced?
5 F2 (g) + 2 NH3 (g) --> N2F4 (g) + 6 HF(g)
a)
268.8 L HF
b)
7.47 L HF
c)
0.54 L HF
d)
134.4 L HF
66.
(a) moles of ammonia are required to produce 134.4 L of dinitrogen tetrafluoride. 5 F2 (g) + 2 NH3 (g) --> N2F4 (g) + 6 HF(g)
67.
How much hydrogen fluoride gas is produced if 200 grams of fluorine and 180 grams of ammonia react?
5 F2 (g) + 2 NH3 (g) --> N2F4 (g) + 6 HF(g)
a)
126.37 grams HF
b)
634.33 grams HF
c)
87.75 grams HF
d)
70.48 grams HF
68.
If 200 grams of fluorine produced 120 grams of hydrogen fluoride gas, the percent yield of the reaction rounded to the nearest whole number is (a) %. 5 F2 (g) + 2 NH3 (g) --> N2F4 (g) + 6 HF(g)
69.
How many grams of iron are needed to produce 140 grams of iron(III) oxide?
4 Fe (s) + 3 O2 (g) --> 2 Fe2O3
a)
97.92 g Fe
b)
24.48 g Fe
c)
122.46 g Fe
d)
150.58 g Fe
70.
How many grams of oxygen are needed to fully react with 223.38 grams of iron?
4 Fe (s) + 3 O2 (g) --> 2 Fe2O3
a)
95.994 g O2
b)
47.997 g O2
c)
170.66 g O2
d)
85.33 g O2
71.
How many moles of iron(III) oxide are produced if 20 moles of iron are reacted in excess oxygen?
4 Fe (s) + 3 O2 (g) --> 2 Fe2O3
(a)
72.
If 60 grams of nitrogen monoxide are reacted in excess ammonia, how much water is produced?
4 NH3 (g) + 6 NO (g) --> 5 N2 (g) + 6 H2O (g)
a)
2.00 mol H2O
b)
1.67 mol H2O
c)
36.02 mol H2O
d)
3.00 mol H2O
73.
How many moles of nitrogen gas are produced if 90 grams of ammonia react with 7 moles of nitrogen monoxide?
4 NH3 (g) + 6 NO (g) --> 5 N2 (g) + 6 H2O (g)
a)
5.83 mol N2
b)
6.61 mol N2
c)
8.4 mol N2
d)
4.28 mol N2
74.
If 800 grams of ammonia react with 2000 grams of nitrogen monoxide, which is the limiting reagent?
4 NH3 (g) + 6 NO (g) --> 5 N2 (g) + 6 H2O (g)
a)
Ammonia
b)
Nitrogen monoxide
75.
How much ammonia is required to produce 22.4 L of water?
4 NH3 (g) + 6 NO (g) --> 5 N2 (g) + 6 H2O (g)
a)
14.93 L NH3
b)
33.6 L NH3
c)
22.4 L NH3
d)
7.47 L NH3
76.
How many moles of nitrogen monoxide are required to produce 10 moles of nitrogen gas?
4 NH3 (g) + 6 NO (g) --> 5 N2 (g) + 6 H2O (g)
a)
12 mol N2
b)
8.33 mol N2
c)
8 mol N2
d)
12.5 mol N2
77.
According to Arrhenius, an acid dissolved in water will
a)
produce hydrogen ions.
b)
produce hydroxide ions.
c)
be a hydrogen-ion donor.
d)
be a hydrogen-ion acceptor.
e)
be an electron-pair acceptor.
78.
According to Bronsted-Lowry theory, a base dissolved in water will
a)
be a hydrogen-ion acceptor.
b)
produce hydrogen ions.
c)
produce hydroxide ions.
d)
be a hydrogen-ion donor.
e)
be an electron-pair acceptor.
79.
According to the Lewis definition, a base dissolved in water will
a)
be an electron-pair donor.
b)
produce hydrogen ions.
c)
produce hydroxide ions.
d)
be a hydrogen-ion donor.
e)
be a hydrogen-ion acceptor.
80.
Determine whether hydrosulfuric acid is monoprotic, diprotic, or triprotic.
a)
Monoprotic
b)
Diprotic
c)
Triprotic
81.
Identify the conjugate base of phosphoric acid when it dissolves in water.
a)
[PO4]3-
b)
[PO3]3-
c)
[P]3-
d)
[H2PO4]1-
82.
Classify water as either an acid or base according to the Bronsted-Lowry definition.
H2O + CH3COO- <---> CH3COOH + OH-
a)
Acid
b)
Base
83.
Classify the acetate ion as either an acid or base according to the Bronsted-Lowry definition.
H2O + CH3COO- <---> CH3COOH + OH-
a)
Acid
b)
Base
84.
How are the concentrations of hydrogen ions (or hydronium ions) and hydroxide ions related in an aqueous solution?
a)
They are inversely proportional.
b)
They are directly proportional.
c)
The product of the concentrations (expressed as molarity [M]) of hydrogen ions and hydroxide ions is 1.0 * 10^-14.
d)
The product of the concentrations (expressed as molarity [M]) of hydrogen ions and hydroxide ions is 1.0 * 10^14.
85.
A solution has a pH of 12. Classify the solution.
a)
Acid
b)
Neutral
c)
Base
86.
A solution has a pH of 5. Classify the solution.
a)
Acid
b)
Neutral
c)
Base
87.
What do we call a substance that changes colors depending the pH of a solution?
a)
pH meter
b)
Acid-base indicator
c)
pH indicator
d)
Color indicator
88.
What is the pH of a solution that has [H+] = 1 x 10^-6 M?
(a)
89.
What is the pH of a solution that has [OH-] = 1 * 10^-11?
(a)
90.
What is [OH-] if a solution has a pH of 12?
a)
1.0 * 10^-2 M
b)
1.0 * 10^2 M
c)
1.0 * 10^12 M
d)
10.0 * 10^-2 M
91.
What determines the strength of acids and bases?
a)
The degree to which they ionize (or dissociate).
b)
The concentration of the acid or base.
c)
Its lifting power.
d)
The volume of the acid or base.
92.
Solution A has a Ka of 5.6 * 10^-2. Solution B has a Ka of 4.8 * 10^-13. Which acid is stronger?
a)
Solution A
b)
Solution B
c)
You cannot tell based on this information.
93.
A 0.5 M solution of a monoprotic acid has a hydronium-ion concentration of 5.77 * 10^-6 M. What is the Ka of this acid?
a)
6.659 * 10^-11
b)
5.77 * 10^-6
c)
1.154 * 10^-5
d)
6.659 * 10^13
94.
Acid HX has a very small Ka. Therefore, we know that the concentration of HX will be much larger than the concentration of H+ or X- at equilibrium.
a)
True.
b)
False.
c)
It's impossible to say given the information.
95.
Write the chemical equation for the ionization of ammonia.
a)
NH3 + H2O <---> (NH4)+ + OH-
b)
NH4 + H2O <---> NH3 + OH-
c)
NH3 + OH- <---> (NH4)+ + H2O
d)
NH3 + NH4 <---> H2O + OH-
96.
A 15M solution of an acid has a Ka of 7.5 * 10^-3. What can you say about this acid?
a)
It is concentrated but weak.
b)
It is dilute and weak.
c)
It is concentrated and strong.
d)
It is dilute but strong.
97.
Identify the products of a neutralization reaction.
a)
A salt
b)
Water
c)
Acid
d)
Base
e)
A gas
98.
When does neutralization occur; that is, when is the equivalence point obtained?
a)
There's an equal number of hydrogen and hydroxide ions in solution.
b)
The number of hydrogen ions is larger than hydroxide ions in solution.
c)
The number of hydroxide ions is larger than hydrogen ions in solution.
99.
How many moles of HCl are required to neutralize an aqueous that contains 0.1 mol Ca(OH)2?
a)
0.2 mol HCl
b)
0.1 mol HCl
c)
0.05 mol HCl
100.
What is the name of the salt you get when you neutralize H3PO4 and Ca(OH)2?
(a)
101.
How many milliliters of 6M sulfuric acid are required to neutralize 3 moles of NaOH? Remember: an x-molar (xM) solution is tells us that there are x moles per 1 liter of solution.
a)
250 mL H2SO4
b)
0.25 mL H2SO4
c)
1000 mL H2SO4
d)
9000 mL H2SO4
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