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WorksheetsHChem Review 1
Total questions: 103
Worksheet time: 5hrs 31mins
Name
Class
Date
1.
What is the molar mass of C6H12O6?
a)
180.18
b)
180.12
c)
180.24
d)
180.06
2.
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
3.
N2 + 3H2 → 2NH3
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
4.
2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
5.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
6.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
7.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
8.
2H2 + O2 → 2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
9.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
10.
O2 + CS2 --> CO2 + SO2
What coefficient would go in front of the O2?
What coefficient would go in front of the O2?
a)
1
b)
2
c)
3
d)
4
11.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
12.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
13.
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
14.
How many grams are in one mole of Oxygen
a)
16
b)
32
c)
15.99
d)
31.98
15.
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
16.
In the reaction 2 H2 + O2 → 2 H2O what is the mole ratio of oxygen to water
a)
1:2
b)
2:1
c)
3:4
d)
4:3
17.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6?
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L
c)
1 mol = 6.02x 1023 particles
d)
more than one
18.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
19.
Which conversion factor should be used to solve the following, "Find the mass in grams of 2.00 x 1023 molecules of F2."
a)
1 mol = 22.4 L
b)
1 mol = 38.00 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
20.
What operation will be performed when converting from moles to another unit?
a)
addition
b)
subtraction
c)
multiplication
d)
division
21.
Which expression below show the correct method of determining the percent composition of Sodium in Na2CO3?
a)
%Na = (22.99g/106g) x 100
b)
%Na = (22.99g/106) / 100
c)
%Na = (45.98g/106g) x 100
d)
%Na = (106/45.98g) x 100
22.
What operation will be performed when converting from a unit to moles.
a)
addition
b)
subtraction
c)
multiplication
d)
division
23.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
24.
The number 6.02 x 1023, which is the number of particles found in a mole.
a)
molar mass
b)
mole
c)
Avogadro's number
d)
hydrate
25.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
26.
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.
27.
What is the empirical formula of the following molecular formula: C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
28.
Which one is empirical?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
29.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
30.
What is the empirical formula of the following molecular formula: C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
31.
Find the percent composition of N2S2.
a)
N: 69.6% S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
32.
To be a neutralization reaction, a reaction MUST
a)
At least contain an acid
b)
At least contain a base
c)
Produce CO2
d)
React an acid with a base, and produce water
33.
Identify this type of reaction:
Al (s) + HCl (aq) → AlCl3 (aq) + H2 (g)
Al (s) + HCl (aq) → AlCl3 (aq) + H2 (g)
a)
Precipitation
b)
Synthesis
c)
Combustion
d)
Single Replacement
34.
The Law of Conservation of Matter states that the total mass of the reactants should be
a)
More than the mass of the products
b)
Equal to the mass of the products
c)
Ignored during the reaction
d)
Less than the mass of the products
35.
Which coefficients are required to correctly balance the equation:
C2S2 + O2 → CO2 + S2O
C2S2 + O2 → CO2 + S2O
a)
1, 2, 3, 2
b)
2, 5, 4, 2
c)
2, 4, 5, 2
d)
2, 3, 5, 2
36.
In the following reaction, what sign is there that a precipitation reaction took place?
AgNO3 (aq) + NaOH (aq) → AgOH (s) + NaNO3 (aq)
AgNO3 (aq) + NaOH (aq) → AgOH (s) + NaNO3 (aq)
a)
The formation of a nitrate
b)
The (aq), meaning aqueous or dissolved in water
c)
The (s), meaning the formation of a solid
d)
The base (OH) reactant
37.
Which of the following reactions involves the ions of two compounds exchanging places to form two new compounds?
a)
Synthesis
b)
Double Replacement
c)
Combustion
d)
Single Replacement
38.
When balancing equations, the rule is that you can only add, change, and remove
a)
Coefficients
b)
Mass
c)
Subscripts
d)
Elements
39.
The formation of water is an example of a ________ reaction because two simple substances (H and O) combine to produce a new compound (H2O).
a)
Single Displacement
b)
Decomposition
c)
Double Replacement
d)
Synthesis
40.
The following reaction is an example of what reaction type?
CoCO3 → CoO + CO2
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
41.
Which of the following reactions involves one element replacing an element in a compound that is from the same activity series?
a)
Double Replacement
b)
Decomposition
c)
Synthesis
d)
Single Replacement
42.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
43.
A + B → AB : is the general form for which reaction type?
a)
Double Replacement
b)
Synthesis
c)
Combustion
d)
Decomposition
44.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
45.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO
N2+O2--> _NO
a)
1
b)
2
c)
3
d)
4
46.
What coefficient goes in the missing blanks? There is only one answer.
SnO2 + __ H2 → Sn + __ H2O
SnO2 + __ H2 → Sn + __ H2O
a)
5
b)
1
c)
3
d)
2
47.
Balance this equation:
__Li + __Cl2 -> __LiCl
__Li + __Cl2 -> __LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
48.
Balance this equation...
HgO --> 2Hg + O2
HgO --> 2Hg + O2
a)
It is balanced
b)
2HgO --> Hg + O2
c)
2HgO --> 2Hg + O2
49.
Which of the following is an unbalanced equation?
a)
CaCO3 --> CaO + CO2
b)
PbO2 + 2H2-->2Pb + H2O
c)
2Na+ 2H2O-->2NaOH + H2
d)
CS2 + 2O2 --> CO2 + 2SO2
50.
Fill in the missing coefficient to balance the equation: Mg + ___ HCl → MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
51.
What is the left part of a chemical equation called?
H2 + O → H2O
H2 + O → H2O
a)
Reactants
b)
Products
c)
Yields
d)
Chemical Equation
52.
What is the right part of a chemical equation called?
H2 + O → H2O
H2 + O → H2O
a)
Reactants
b)
Products
c)
Yields
d)
Chemical Equation
53.
Si + S8 →Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
54.
Ca + AlCl3→ CaCl2 + Al
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
55.
KOH + H3PO4 → K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
56.
What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)
a)
0.8 M
b)
1.5M
c)
3.0M
d)
6.0M
57.
What is the molarity of a solution when 80.0 g of sodium chloride (NaCl) are dissolved in 500.0 ml of water
a)
1.37M
b)
1.45 M
c)
2.74M
d)
6.25M
58.
A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility
a)
lowering the temperature of the solvent
b)
stirring the solute in the solution
c)
increasing the pressure on the solution
d)
increasing the particle size of the solute
59.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
60.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
61.
What is the minimum temperature needed to dissolve at least 10 g of KClO3?
a)
25 ⁰C
b)
10 ⁰C
c)
5 ⁰C
d)
100 ⁰C
62.
How many grams of sodium nitrate, NaNO3, are soluble in 100 g of water at 10 ºC?
a)
80 grams
b)
100 grams
c)
40 grams
d)
10 grams
63.
When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
64.
When 30 grams of potassium nitrate, KNO3, is dissolved in 100 grams of water at 20 ºC, the solution can be correctly described as:
a)
saturated
b)
unsaturated
c)
supersaturated
65.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water.
a)
3
b)
1
c)
6
d)
9
66.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.07 gram
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
67.
What is the molality of a solution containing 1.3 mol in 13.4 kg of solution?
a)
9.7 m
b)
17.42 m
c)
0.097 m
68.
What is the molality of 1.2 g of HCl in 750 g of solution?
a)
0.04 m
b)
0.00004 m
c)
0.0016 m
69.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
70.
What is the percent-by-mass, concentration of sucrose in a solution made by dissolving 7.6 g of sucrose in 83.4 g of water?
a)
0.0835
b)
2.78
c)
8.35
d)
0.0278
71.
What mass, in grams, of sodium sulfate is needed to make 275 g of a 1.5% aqueous solution of sodium sulfate?
a)
6.0
b)
7.5
c)
4.1
d)
2.2
72.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
73.
How many milliliters of concentrated 18M H2SO4 is needed to prepare 250 mL of a 6.0 M solution?
a)
83.3 mL
b)
0.083 L
c)
1500 mL
d)
1.5 L
74.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 and to 500. mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
75.
Colligative properties of solutions are those properties that depend on
a)
the amount of solute only
b)
the identity of solute only
c)
both the identity and the amount of solute
76.
The freezing point of a solution is ___________ that of a pure solvent
a)
more than
b)
less than
c)
equal to
77.
The boiling point of a solution is ___________ that of a pure solvent
a)
more than
b)
less than
c)
equal to
78.
The vapor pressure of a pure solvent is ___________ that of a solution
a)
more than
b)
less than
c)
equal to
79.
Ionic solutes causes the vapor pressure to
a)
lower more than molecular ones
b)
lower less than molecular ones
c)
lower as much as the molecular ones do
80.
The temperature at which the vapor pressure of the liquid phase equals atmospheric pressure is called
a)
Boiling point
b)
Melting point
c)
Freezing point
81.
The higher the number of solute particles in a solution,
a)
the lower the vapor pressure
b)
the lower the freezing point
c)
the higher the boiling point
d)
all of the above
82.
Calculate the approximate boiling point (in oC) of a solution of 285 g of magnesium chloride in 2.0 kg of water. (Kb=0.51 oC/m)
a)
103.1 oC
b)
101.6 oC
c)
102.3 oC
d)
104.8 oC
83.
Endothermic reactions feel
a)
warm
b)
cold
84.
Exothermic reactions feel
a)
warm
b)
cold
85.
energy in endothermic reactions are
a)
released
b)
ended
c)
absorbed
86.
energy in exothermic reactions are
a)
released
b)
absorbed
87.
Heat is measured in
a)
joules
b)
grams
c)
degrees celcius
88.
q stands for which variable
a)
heat
b)
mass
c)
specific heat
d)
change in temperature
89.
The variable C stands for what
a)
heat
b)
mass
c)
specific heat
d)
change in temperature
90.
For the formula:
Q= m c ∆T
The units for specific heat are:
Q= m c ∆T
The units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
91.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of .10 J/g°C, what is the mass of the iron sample?
a)
25g
b)
30g
c)
20g
d)
50g
92.
If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal? (show your work)
a)
2.34 J/g°C
b)
0.472 J/g°C
c)
6.13 J/g°C
d)
0.163 J/g°C
93.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
94.
If you add a ice that is -10 degrees Celcius to a cup of water that is 0 degrees Celcius, what will happen?
a)
Ice will melt
b)
Ice will get larger
c)
Ice will stay the same
d)
Ice will catches on fire
95.
When 1500J of energy is lost from a 120 gram object, the temperature decreased from 45 degrees C to 40 degrees C. What is the specific heat of the object?
a)
2.5 J/gC
b)
1.5 J
c)
12.5 Cal/gC
d)
15 J/gC1
96.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
97.
How much energy must be used to produce 4.75 mol of gaseous water?
H2O (l) + 44.0 kJ --> H2O (g)
H2O (l) + 44.0 kJ --> H2O (g)
a)
207 kJ
b)
9.36 kJ
c)
206.8 kJ
d)
9.362 kJ
98.
4 PCl5 + 3438 kJ --> P4 + 10 Cl2
How much energy is required to produce each mole of chlorine?
How much energy is required to produce each mole of chlorine?
a)
687.6 kJ
b)
859.5 kJ
c)
343.8 kJ
d)
245.8 kJ
99.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
100.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
101.
What is the latent heat of fusion of lead (in joules per gram), if 6.30 kilojoules of heat are required to convert 255 grams of solid lead at its melting point into a liquid?
a)
.025
b)
1.61
c)
24.7
d)
40.5
102.
What letter represents boiling?
a)
B
b)
C
c)
D
d)
E
103.
What letter represents a liquid being heated?
a)
A
b)
B
c)
C
d)
D
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