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Semester 2 Exam Study Guide

Total questions: 66

Worksheet time: 2hrs 6mins

Name
Class
Date
1.
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
2.
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
3.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
4.

4NH3 + 5O2 --> 4NO + 6H2O

How many grams of NO are formed if 6.30g of ammonia react with 3.6g of oxygen?

a)

0.37g

b)

2.70g

c)

1.35g

d)

11.1g

5.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
6.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
7.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)

456 grams

d)
462 grams
8.
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
9.
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   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
10.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
11.
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)
749 g
b)
225 g
c)
479 g
d)
814 g
12.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
13.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

14.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron can be made from 6 moles H2 and excess Fe2O3?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

15.
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
16.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
17.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
18.
Identify the phosphide ion
a)
P5+
b)
P3+
c)
P3-
d)
P4-
19.
What is the name for the NO3- ion?
a)
nitrate ion
b)
nitrite ion
c)
nitrogan ion
d)
nitride ion
20.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
21.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
22.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
23.
What is the metallic ion in the compound CuCl?
a)
Cu1+
b)
Cu2+
c)
Cu1-
d)
Cu2-
24.
What is the formula for barium hydride?
a)
BaOH2
b)
Ba(OH)2
c)
BaH2
d)
BaOH
25.
Name the compound Mg3(PO4)2
a)
magnesium phosphate
b)
magnesium (III) phosphate
c)
magnesium phosphite
d)
magnesium phosphide
26.
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 
27.
carbonic acid
a)
H2CO3
b)
H2CrO4
c)
H2C2O4
d)
HCO3
28.
HI
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
29.
HF
a)
flouric acid
b)
hydrofluoric acid
c)
fluorate acid
d)
hydrogen fluoridic acid
30.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
31.
Acids react with
a)
water to produce bases and salts
b)
salts to produce bases and water
c)
neither bases, salts nor water
d)
bases to produce salts and water
32.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

33.

A sour taste is a characteristic of:

a)

acids

b)

bases

c)

neutral

d)

pH scale

34.

For the following reaction, determine which species is acting as the Arrhenius acid:

HCl + KOH --> KCl + H2O

a)

HCl

b)

KOH

c)

KCl

d)

H2O

35.

In the following reaction, determine which species is the salt:

HCl + KOH --> KCl + H2O

a)

HCl

b)

KOH

c)

KCl

d)

H2O

36.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

37.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

38.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
39.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

40.
Calculate the partial pressure of H2 at 20oC when the vapor pressure of water is 17.5torr. The total pressure of the gases is 750torr.
a)
767.5torr
b)
732torr
c)
42.86torr
41.

Which is a characteristic of a base?

a)

tastes sour

b)

found mostly in foods

c)

feels slippery

d)

turn litmus paper red

42.

According to Arrhenius, what is the definition of an ACID?

a)

a substance that contains hydroxide and ionizes to produce OH-

b)

a substance that contains hydrogen and ionizes to produce H+

c)

a substance that contains hydrogen and ionizes to produce OH-

d)

a substance that contains hydroxide and ionizes to produce H+

43.

Which of the following will conduct electricity? Select all that apply

a)

Acidic solutions

b)

Basic solutions

c)

Ionic solutions

d)

Neutral covalent solutions

44.

Neutralization is the process of an acid and a base reacting to form what? Select all that apply

a)

An ionic salt

b)

Hydronium ions

c)

NaCl

d)

Water

45.
If a solution has a [H+] of 1.2 x 10-4M what is the [OH-]?
a)
8.3 x 10-4M 
b)
8.3 x 10-11M 
c)
1.2 x 1010M 
d)
1.2 x 10-4M 
46.
If a solution has a [OH-] of 3.42 x 10-12M what is the [H+]?
a)
2.92 x 10-3M 
b)
3.42 x 102M 
c)
2.92 x 10-2M 
d)
3.42 x 10-5M 
47.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
48.
Which accepts protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
49.
What substances increase H+ ion concentrations when dissolved in water?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
50.
What substances increase OH- ion concentrations when dissolved in water?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
51.
Which donates protons?
a)
Brønsted-Lowry Acids
b)
Brønsted-Lowry Bases
c)
Arrhenius Acids
d)
Arrhenius Bases
52.
When citric acid is produced by the cells of an orange and dissolves in water, it produces a relatively small number of hydronium ions. Citric acid is best described as a
a)
concentrated acid. 
b)
weak acid. 
c)
dilute acid.
d)
strong acid.
53.

Accepts a pair of electrons

a)

Lewis Acid

b)

Lewis Base

c)

Bronsted Lowry Acid

d)

Arrhenius Base

54.

Lewis bases are defined as

a)

H+ acceptors

b)

electron pair acceptors

c)

H+ donors

d)

electron pair donors

55.

Which is the correct set of acid properties?

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

56.

Which of the following show an acid and its conjugate base pair (in that order)

a)

H2SO4, SO42-

b)

OH-, H2O

c)

NH4+, H2O

d)

H2CO3, HCO3-

57.
Which of the following shows the correct conjugate acid base pair?
a)
HCI (acid) / H3O+ (conjugate base)
b)
HCI (acid) / CI- (conjugate base)
c)
HCI (base) / CI- (conjugate acid)
d)
HCI (base) / H3O+ (conjugate acid)
58.

NH3 + H2O --> NH4+ + OH-

What is NH4+ in this reaction?

a)

acid

b)

base

c)

conjugate acid

d)

conjugate base

59.

In the equation below, what is the conjugate base?

HBr + H2O ↔ Br- + H3O+

a)

HBr

b)

H2O

c)

Br-

d)

H3O+

60.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

61.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

62.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

63.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

64.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

65.
The [H+] is orange juice is
0.00020 M.  FInd the pH of orange juice.
a)
1
b)
3.7
c)
10.3
d)
13
66.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M

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