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WorksheetsChemistry Finals Review 2
Total questions: 61
Worksheet time: 15hrs 15mins
Name
Class
Date
1.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25
d)
1.91 x 1022
2.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
3.
Determine the number of
atoms in
2.50 moles of zinc.
atoms in
2.50 moles of zinc.
a)
1.51 x 1024 atoms
b)
4.15 x 10-24 atoms
c)
2.71 x 10-22 atoms
d)
163 atoms
4.
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
5.
Find the number of moles in 30 grams of H3PO4
a)
30 mol H3PO4
b)
0.31 mol H3PO4
c)
97 mol H3PO4
d)
3.26 mol H3PO4
6.
How many moles are in 564 grams of Copper?
a)
0.11 mol Cu
b)
25 mol CU
c)
87 mol Copper
d)
8.87mol Cu
7.
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
8.
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
9.
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
10.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
11.
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
12.
CaC₂(s) + 2H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
13.
How many grams are in one mole of Oxygen
a)
16
b)
32
c)
15.99
d)
31.98
14.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
15.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
16.
If 3.0 moles of Al(NO3)3 are used up in the following balanced reaction, how many moles of HNO3 will be produced?
2 Al(NO3)3(aq) + 3 H2SO4(aq) --> Al2(SO4)3(s) + 6 HNO3(aq)
2 Al(NO3)3(aq) + 3 H2SO4(aq) --> Al2(SO4)3(s) + 6 HNO3(aq)
a)
9.0 moles
b)
6.0 moles
c)
3.0 moles
d)
2.0 moles
17.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction.
18.
The substances at the beginning of a chemical equation are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
19.
Balance this equation
_N2 + _H2 --> _NH3
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
20.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
21.
Balance this equation.
_SnO2 +_H2-->_Sn +_H2O
_SnO2 +_H2-->_Sn +_H2O
a)
1,1,2,1
b)
1,2,1,1
c)
1,2,1,2
d)
1,2,2,1
22.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
23.
What percent of CuCl2 is Cu?
a)
47.27%
b)
52.73%
c)
89.63%
d)
33%
24.
What percent of magnesium bromide, MgBr2, is magnesium?
a)
13.19%
b)
86.8%
c)
7.58%
d)
13.20%
25.
How many moles are in 88 g of propane, C3H8.
a)
2.0
b)
16.0
c)
0.051
d)
3,872
26.
What is the molecular formula of a compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole?
a)
C2O4H8
b)
C8O2H4
c)
C4O2H8
d)
C4O8H2
27.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
28.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
29.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
30.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
31.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water?
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
32.
Which is an example of a solute?
a)
Egg whites
b)
Sugar
c)
Water
d)
Acetone
33.
Which is an example of a solvent?
a)
Salt
b)
Egg whites
c)
Water
d)
Sugar
34.
The amount of solute dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
35.
As we dilute a solution.....
a)
The volume increases and the molarity (M) increases
b)
The volume increases and the molarity (M) decreases
c)
The volume decreases and the molarity (M) increases
d)
The volume decreases and the molarity (M) decreases
36.
How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?
a)
7.5 mL
b)
15 mL
c)
1333 mL
d)
200 mL
37.
If I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if I add 560 mL more water to it?
a)
.188 M
b)
3.78 M
c)
.389 M
d)
1.76 M
38.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
.278 mL
c)
2.8 mL
d)
278 mL
39.
30cm3 of NaOH is neutralised by 12.3cm3 of 0.2mol/l HCl. What is the concentration of the NaOH.
a)
82 mol/l
b)
0.82 mol/l
c)
0.49 mol/l
d)
0.082 mol/l
40.
The reaction of perchloric acid (HClO4) with lithium hydroxide (KOH) is described by the equation
HClO4 + KOH → KClO4 + H2O
Suppose 100 mL of perchloric acid is neutralized by exactly 50,0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?
HClO4 + KOH → KClO4 + H2O
Suppose 100 mL of perchloric acid is neutralized by exactly 50,0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?
a)
0.5M
b)
50M
c)
2.0M
d)
1.0M
41.
The reaction of sulfuric acid (H2SO4) with Sodium hydroxide (NaOH) is described by the equation:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
Suppose 50 mL of NaOH with unknown concentration is placed in a flask with bromthymol blue indicator. A solution of 0.20 M H2SO4 is dripped into the NaOH solution. After exactly 25.0 mL of H2SO4 is added, the indicator changes from blue to yellow. What is the concentration of the KOH?
H2SO4 + 2NaOH → Na2SO4 + 2H2O
Suppose 50 mL of NaOH with unknown concentration is placed in a flask with bromthymol blue indicator. A solution of 0.20 M H2SO4 is dripped into the NaOH solution. After exactly 25.0 mL of H2SO4 is added, the indicator changes from blue to yellow. What is the concentration of the KOH?
a)
0.20M
b)
4.0M
c)
2.5M
d)
0.4M
42.
Complete the following reaction:
HCl + Mg(OH)2 -->
a)
MgCl2 + H2O
b)
Mg +H2O
c)
MgCl2 + H2
d)
MgCl2 + H2O + CO2
43.
Identify the salt in the following equation:
Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2
Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
44.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M
d)
0.30 M
45.
What is unsaturated?
a)
A solution with more solute than solvent
b)
A solution with less than the maximum amount of solutes
c)
A solution with the perfect balance of solutes and solvents
d)
A solution with solids at the bottom
46.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
47.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
48.
which is supersaturated at 60 g and 60 degrees Celsius
a)
KCLO3
b)
KNO3
c)
NaCl
d)
NaNO3
49.
Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.
a)
Volume
b)
Proportion
c)
Mass
d)
Particles
50.
How many more grams of KNO3 dissolve at 50 ⁰C compared to 0 ⁰C?
a)
85 g
b)
15 g
c)
70 g
d)
100 g
51.
How many grams of SO2 can dissolve at 50 ⁰C?
a)
5 g
b)
10 g
c)
20 g
d)
39 g
52.
What is a precipitate?
a)
an insoluble reactant formed during a chemical reaction
b)
an insoluble product formed during a chemical reaction
c)
a soluble solvent in a saturated solution
d)
a soluble solute in a saturated solution
53.
NH4NO3
a)
soluble
b)
insoluble
54.
AgCl
a)
soluble
b)
insoluble
55.
K2SO4
a)
soluble
b)
insoluble
56.
FeS
a)
soluble
b)
insoluble
57.
BaSO4
a)
soluble
b)
insoluble
58.
K2CO3
a)
soluble
b)
insoluble
59.
CaCO3
a)
soluble
b)
insoluble
60.
How much C12H22O11 solute is saturated at 40 degrees?
a)
240
b)
220
c)
230
d)
250
61.
How much NaBr solute is saturated at 70 degrees?
a)
110
b)
120
c)
130
d)
140
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