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Chemistry CBA Review

Total questions: 81

Worksheet time: 2hrs 11mins

Name
Class
Date
1.

The ideal gas law equation can be used to find all of the following except...

a)

number of moles of gas

b)

volume of a gas

c)

pressure of a gas

d)

temperature of a gas

e)

how much of a different chemical will be formed

2.

In order to use gas stoichiometry....(click all that apply)

a)

You must know the amounts of all the reactants

b)

The conditions must be STP

c)

You can use 1 mole = 22.4 L to convert between moles and liters

d)

Both chemicals you are relating must be gases

3.

If you know the temperature, pressure and volume of a gas, how would you find the number of moles of gas?

a)

n = PV/RT

b)

gas stoichiometry

c)

1 mole = 22.4L

d)

1 mole = molar mass

4.

Stoichiometry...

a)

is used to relate two chemicals in a balanced equation

b)

can only be used if we know the number of grams of a substance

c)

only relates grams to grams

d)

can be used to find moles, pressure or volume

5.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
6.

151 grams of Al2O3 are produced. How many grams of Al was needed in the reaction? Al + O2 -------> Al2O3 balance first.

a)

79.91 g

b)

22.4 liters

c)

57.8 g

d)

142.8 g

7.

What does R stand for

a)

Ideal gas constant

b)

Molar constant

c)

Temperature constant

d)

Ideal gas law

8.

What does the variable "n" represent in the ideal gas law?

a)

pressure

b)

volume

c)

moles

d)

temperature

9.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
10.

Which of the following variables is NOT correctly matched with its value for this problem:

What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

a)

V = 4.2 L

b)

R = 0.0821 L⋅atm∕mol⋅K

c)

n = 0.023 mol

d)

P = 20⁰C

11.
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
12.

Using the balanced equation,
Mg(s)   +   2HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many moles of HCl are consumed by the reaction with 2.50 moles of magnesium?

a)

5.00 moles

b)

2.50 moles

c)

120 moles

d)

60 moles

13.

Using the balanced equation,
Mg(s)   +  2 HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many moles of H₂ gas are formed when 4.0 moles of HCl is added to the reaction?

a)

2 moles

b)

4 moles

c)

8 moles

d)

1 mole

14.

Which choice is the fromula for calculating percent by mass?

a)

a

b)

b

c)

c

d)

d

15.
a)

16.00

b)

1.01

c)

17.01

d)

18.02

16.

a)

5.60%

b)

11.20%

c)

88.79%

d)

18.02%

17.

a)

27.29%

b)

36.35%

c)

72.27%

d)

1.34%

18.

a)

27.29%

b)

36.35%

c)

72.27%

d)

1.34%

19.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
20.

How many moles of copper are 4.57 x 1013 atoms of copper?

a)

7.59 x 10-11 moles

b)

2.75 x 1037 moles

c)

7.59 x 1011 moles

d)

2.75 x 10-37 moles

21.

1 mole of zinc is how many atoms?

a)

65.4

b)

6.02x1023

c)

6.54x1023

d)

0.000,000,000,000,000,000,000,654

22.

What is the mass of one mole of water (H2O)?

a)

18 g/mol

b)

16 g/mol

c)

1 g/mol

d)

6.022x10^23 atoms

23.

How many atoms are in 117.3 grams of Potassium? Hint: Look at the periodic table and use your calculator

a)

1.80x1024 atoms

b)

39.1 atoms

c)

3 atoms

d)

6.02x1023 atoms

24.

How many moles are in 16.94 g of water? (hint: do you know the formula for water?)

a)

16.94 moles

b)

0.9403 mole

c)

305.2 moles

d)

1.063 moles

25.

If you want 1.55 moles of nitrogen trichloride, how many grams should you measure out?

a)

0.0129 g

b)

120. g

c)

187 g

d)

9.33 g

26.

How many water molecules are in 5.2 moles of water?

a)

6.0 x 1023 molecules

b)

5.2 molecules

c)

3.1 x 1024 molecules

d)

8.6 x 10-24 molecules

27.
How many Aluminum are in Al2O3?
a)
3
b)
2
c)
5
28.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
29.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
30.

Calculate the number of Oxygen atoms in Al(OH)3

a)

1

b)

2

c)

3

d)

4

31.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
32.

4CF2Cl2

a)

C = 4, F = 4, Cl = 2

b)

C = 1, F = 8, Cl = 8

c)

C = 4, F = 8, Cl = 8

d)

C = 1, F = 4, Cl = 8

33.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

34.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

35.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

36.

Isotopes are atoms of the same element with different ____________.

a)

Number of Neutrons & Mass Number

b)

Number of Protons & Atomic Number

c)

Number of Protons, Neutrons, and Electrons

d)

Number of Electrons & Mass Number

37.

_______ is the average mass of all the isotopes of an element.

a)

Atomic Mass

b)

Atomic Number

c)

Chemical Symbol

d)

Element Name

38.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
39.

How do you calculate the atomic weight of an element with two isotopes, if the isotopic masses and their natural abundances are given? For example, if isotope A has a mass of 10 amu and 20% abundance, and isotope B has a mass of 11 amu and 80% abundance.

a)

10×0.2+11×0.82\frac{10 \times 0.2 + 11 \times 0.8}{2}

b)

10×0.2+11×0.810 \times 0.2 + 11 \times 0.8

c)

10+112\frac{10 + 11}{2}

d)

(10×0.2)+(11×0.8)\left(10\times0.2\right)+\left(11\times0.8\right)

40.

H3PO4 + KOH ------> K3PO4 + H2O


Is this equation balanced?

a)

yes

b)

no

c)

impossible to determine

41.

Choose the answer that shows this equation balanced:


C + S8 ----->CS2

a)

4C + S8 ----->4CS2

b)

3C + S8 -----> 2CS2

c)

C + 2S8 -----> 6CS2

d)

8C + S8 -----> 4CS2

42.

Choose the answer that shows this equation Balanced


N2 + O2 ----> N2O5

a)

3N2 + O2 ----> 3N2O5

b)

5N2 + 2O2 ----> 5N2O5

c)

2N2 + 5O2 ----> 2N2O5

d)

Cannot be balanced

43.

Which choice shows this equation balanced?


K + B2O3 -----> K2O + B

a)

2K + B2O3 -----> K2O + 3B

b)

K + 2B2O3 -----> 4K2O + B

c)

6K + B2O3 -----> 3K2O + 2B

d)

balanced as is.

44.
What is the charge of Aluminium?
a)
3
b)
+3
c)
+2
d)
+1
45.
Atoms that lose electrons become...
a)
negatively charged
b)
postively charged
c)
remain neutral, no charge
d)
losers
46.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
47.
If an atom gains 3 electrons, what charge will it have as an ion?
a)
+3
b)
-3
c)
+5
d)
-5
48.
If an element gains 2 electrons, what charge will it have when it becomes an ion?
a)
+2
b)
-2
c)
-6
d)
-6
49.
If an atom loses 2 valence electrons, what charge will it have as an ion?
a)
+2
b)
-2
c)
0
d)
+8
50.
If an atom loses 2 valence electrons, what charge will it have as an ion?
a)
+2
b)
-2
c)
0
d)
+8
51.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

52.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

53.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

54.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

55.
MgS 
a)
Magnesium sulfide
b)
Monomagnesium monosulfide
c)
Magnesium monosulfide
56.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

57.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

58.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

59.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
60.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
61.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
62.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
63.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
64.
SiCl4
a)
silicon tetrachloride
b)
silicon quadchloride
c)
monosilicon tetrachloride
d)
silicon chloride
65.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
66.
How many valence electrons are in an atom of Se?
a)
2
b)
8
c)
6
d)
5
67.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
68.
How many valence electrons are in an atom of P?
a)
4
b)
5
c)
2
d)
3
69.
How many valence electrons are found in atoms of group 15?
a)
4
b)
5
c)
2
d)
3
70.
How many valence electrons are found in atoms of Calcium?
a)
4
b)
5
c)
2
d)
3
71.
Which statement is not a description of a chemical reaction?
a)
A solid is dropped into a beaker of liquid and a gas is released.
b)
Two liquids are mixed in a beaker and a solid forms at the bottom of the beaker.
c)
A solid is dropped into a beaker of liquid and an explosion occurs.
d)
A liquid is heated in the sun and half of it evaporates.
72.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
73.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
74.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
75.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

76.

Combustion reactions will always involve

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy

d)

CO and H2O

77.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

78.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
79.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
80.

Is this the correct structure for CH2O?

a)

Yes

b)

No

81.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)

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