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Semester 2 - General Review

Total questions: 97

Worksheet time: 3hrs 58mins

Name
Class
Date
1.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
2.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
3.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
4.
What is the molar mass of C2H4O2?
a)
40g
b)
50g
c)
60g
d)
68g
5.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
6.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
7.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
8.
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
9.
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
10.
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
11.
Which would have more atoms?
a)

1 mole of Li

b)

1 mole of Au

c)

1 mole of Si

d)

None, all are equal

12.

If 55.6 grams of calcium carbonate react in excess sodium hydroxide, how many grams of Na2CO3 are made?

Reaction: CaCO3 + NaOH → Ca(OH)2 + Na2CO3

a)

147.34 gram

b)

52.45 gram

c)

55.9 gram

d)

194.24 gram

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? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
14.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

15.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
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.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
17.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
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
18.
Mg(s) + 2 HCl(aq)  -->  MgCl₂(aq)   + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
19.
Balance the following reaction :
 
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
20.
 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?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
21.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
22.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
23.
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
24.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
25.

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

a)

Percent

b)

actual

c)

stoichiometry

d)

theoretical

26.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
27.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
28.

Solid or liquid that is being dissolved? (a)  

Choose from the below words
solute
solvent
solution
solubility
29.
The thing that does the dissolving
a)
Solute
b)
Solvent
c)
Colloid
d)
Solution
30.
Water is a universal solvent
a)
true
b)
false
31.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
32.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
33.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
34.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
35.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
36.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

37.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
38.
Does HCl have hydrogen bonding?
a)
yes
b)
no
39.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
40.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
41.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

42.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

43.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

44.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

45.

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

46.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

47.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

48.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

a)

1.6 M

b)

0.63 M

c)

10 M

d)

2.6 M

49.

What is the meaning of standard solution?

a)

A solution of which its concentration does not accurately known.

b)

Measurement that shows the quantity of solute in one unit of volume of solution

c)

A solution of which its concentration is accurately known.

d)

Concentration that shows the number of mol of solute

50.

In dilution method, ___________increase but the_____________ remains constant.

a)

volume of solvent

b)

concentration

c)

mass

d)

number of moles of solute

51.

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

52.

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

53.

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

54.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)

Combination/Synthesis

b)
Decomposition
c)

Single Displacement

d)

Double Displacement

55.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)

Combination/Synthesis

b)
Decomposition
c)

Single Displacement

d)

Double Displacement

56.
What is decomposition?
a)
putting substances together
b)
breaking substances apart
c)

element displacing another element in a compound

d)

burning of a substance

57.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)

Combination/Synthesis

d)

Single Displacement 

58.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
59.

What type of reaction is taking place in this picture?

a)

Combination/Synthesis

b)
Decomposition
c)

Single Displacement

d)

Double Displacement

60.
4Si   + S8   -->   2Si2S4
a)

Combination/Synthesis

b)
Decomposition
c)
Single Displacement
d)
Double Displacement
61.

What reaction has the following general formula:

AB + CD --> CB + AD

a)

Combination/Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

62.

When solutions of MgCO3 and Fe2(SO4)3 are combined, what precipitate(s) forms?

a)

MgSO4

b)

neither form a precipitate

c)

MgSO4 and Fe2(CO3)3

d)

Fe2(CO3)3

63.

Identify the spectator ion(s) in the equation: 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) --> Ag2S(s) + 2Na+(aq) + 2NO3–(aq)

a)

2Ag+(aq) + 2NO3–(aq)

b)

2Na+(aq) + 2NO3–

c)

2Na+(aq) + S2–(aq)

d)

Ag2S(s) + 2Na+(aq

64.

Which of the following best describes a precipitate?

a)

an insoluble solid

b)

a soluble solid

c)

a soluble gas

d)

an insoluble liquid

65.

AB (aq) + CD (aq) → AD (aq) + CB(s)


Which substance is the precipitate in the reaction above?

a)

AB

b)

CD

c)

AD

d)

CB

66.

Use the Solubility Rules to determine if the following compound is soluble in water:


Li2S

a)

Soluble

b)

Insoluble

67.

Based on the activity series, will this reaction occur?

Ni (s) + HCl (aq) →

a)

Yes

b)

No

68.

Based on the activity series, will this reaction occur?

Au (s) + HCl (aq) →

a)

Yes

b)

No

69.

Based on the activity series, will this reaction occur?

Sr (s) + HCl (aq) →

a)

Yes

b)

No

70.

The pH scale is an inverse function. This means the ___________ the concentration of hydrogen ions, the ___________ the pH is. (select all that apply)

a)

higher, lower

b)

lower, higher

c)

higher, higher

d)

lower, lower

71.

Substances with a pH of 7 are

a)

Acidic

b)

Basic

c)

Neutral

d)

Saturated

72.

If we add EQUAL amounts of equally strong Acid and Base to a solution, we call this

a)

Supersaturated

b)

Dangerous

c)

Neutralization

d)

Dilution

73.

Choose the substance that is more acidic using the scale

a)

Milk

b)

Soap

c)

Coffee

d)

Stomach acid

74.

What would be the two new compounds that would be formed in this reaction?

HCl + NaOH -> ______? + ______?

a)

NaCl

b)

ClOH

c)

HNa

d)

H2O

75.

HBr is an example of a(n)

a)

Acid

b)

Base

c)

Neutral

76.

Ca(OH)2 is an example of a(n)

a)

Acid

b)

Base

c)

Neutral

77.

This substance releases OH- into solution

a)

Acid

b)

Base

c)

Neutral

78.

Which solution releases H+ in solution?

a)

Base

b)

Acid

c)

Buffer

d)

Water

79.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
80.

A type of chemical that forms solutions that taste sour, due to high concentrations of positive hydrogen ions

a)

acid

b)

base

c)

salt

d)

pH

81.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
82.
NaCl is a ...
a)
acid
b)
base
c)
salt
d)
water
83.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

84.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

85.

Which of these titres are concordant?

a)

12.7cm3

b)

12.3cm3

c)

12.4cm3

d)

12.0cm3

86.

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

87.
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?
a)
0.5M
b)
50M
c)
2.0M
d)
1.0M
88.
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?
a)
0.20M
b)
4.0M
c)
2.5M
d)
0.4M
89.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing total surface area

d)

All of these

90.

List three factors that affect the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

91.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
92.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
93.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
94.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
95.

At what time the volume of product reach 35 cm3

a)

0

b)

100

c)

20

d)

60

96.

The graph below shows how the concentration of a reactant in four different reactions changes over time. Which reaction is the slowest?

a)

A, blue

b)

B, red

c)

C, green

d)

D, purple

97.

In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulfuric acid.The solid line on the graph shows the volume of gas given off when the 2 g lump is used.


Which dotted line is obtained when the zinc is powdered?

a)

A

b)

B

c)

C

d)

D

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