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Second Semester Exam

Total questions: 91

Worksheet time: 2hrs 13mins

Name
Class
Date
1.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
2.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
3.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
4.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
5.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
6.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
7.

What units are used to measure volume? CHECK ALL CORRECT ANSWERS

a)

Liters

b)

mL

c)

L

d)

Kelvin

e)

Celsius

8.

A balloon with 3L of air starts at a pressure of 233 kPa, then it rises several thousand feet to a pressure of 190 kPa. Which gas law would let you solve for the new volume?

a)
b)
c)
d)
9.

10. A 500L container filled with a gas. This gas heated from 200K to 400K. If the pressure remains constant, what is the new volume of the container?

a)

250 L

b)

1000 L

c)

500 L

d)

2000 L

10.

A gas occupies 900.0 mL at a temperature of 27.0 °C. What is the volume at 132.0 °C?

(a)  

11.

What is the variable for V for idea gas laws

a)

mm Hg

b)

mL

c)

gallons

d)

L

12.

How do you convert from oC to K

(a)  

13.

Which is a correct unit for R?

a)

L.atm/mol.k

b)

L.atm

c)

mmHg/mol.K

d)

L.atom/mol

14.

1 atm =

a)

760 mm Hg

b)

920 mm Hg

c)

102 mm Hg

d)

786 mm Hg

15.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
16.
If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?
a)
1.75 atm
b)
1.8 atm
c)
1.3 atm
d)
1.29 atm
17.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
18.
A sample of a gas has a volume of 852 mL at 298 K. What temperature is necessary for the gas to have a volume of 945 mL?
a)
57.5⁰C
b)
57.5 K
c)
331 K
d)
330 ⁰C
19.
A sample of oxygen at 28.0°C has 340.0 kPa. What will its temperature be at 150.0 kPa?
a)
132.8 K
b)
132.8 °C
c)
682.2 K
d)
12.35 K
20.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
d)
Left side is balanced
21.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
22.
Which problem is balanced?
a)
PbO2 + 2H2--> H2SO4
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
d)
2Na + 2H2O --> 2NaOH + H
23.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
24.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
25.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
26.
Finish a blalanced equation:
Mg(OH)2 --> __________
a)
Mg(OH)2 --> MgOH
b)
Mg(OH)2 --> MgO+ H2O
c)
Mg(OH)2 --> MgO+ H2
d)
Mg(OH)2 --> Mg+ H2O
27.
Balance this equation:
P4+O2  -->  P2O3
a)
3 P4+ O2 --> 2 P2O3
b)
 P4+ O2 --> 2 P2O3
c)
 P4+ 3 O2 --> 2 P2O3
d)
 P4+ 2 O2 --> 3 P2O3
28.
Balance this equation,            
Al2O3 --> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 --> 2Al+3O2 
c)
2Al2O3--> 4Al+3O2 
d)
3Al2O3--> 2Al+O2 
29.
Which elements are(is) not balanced?
LiNO3 +CaBr2 --> Ca(NO3)2 +  LiBr   
a)
Li
b)
Ca and Li
c)
O and N
d)
Ca
30.
Balance the equation:
Si(OH)4+NaBr--> SiBr4+NaOH
a)
Si(OH)4+2NaBr--> SiBr4+NaOH
b)
Si(OH)4+4NaBr--> SiBr4+4NaOH
c)
Si(OH)4+NaBr--> SiBr4+4NaOH
d)
Si(OH)4+2NaBr--> SiBr4+2NaOH
31.

Balance this equation.

__SnO2 +__H2-->__Sn +__H2O

a)

1,1,2,1

b)

1,2,1,1

c)

1,2,1,2

d)

1,2,2,1

32.

Balance this equation.

__CF4 + __Br2 --> __CBr4 + __F2

a)

2,1,2,1

b)

1,2,2,1

c)

1,2,1,2

d)

2,2,2,2

33.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
34.

Balance this equation.

__Mg + __Cl2 --> __MgCl2

a)

1, 2,1

b)

already balanced

c)

2,1,1

d)

1,1,2

35.

What coefficient should be used to make the following equation balanced?

N2+O2--> __?__NO

a)

1

b)

2

c)

3

d)

4

36.

Drag and drop the coefficients that balance this equation 2 FeFe   + ​ (a)   Cl2Cl_2  ---->  ​ (b)     FeCl3FeCl_3  

Choose from the below words
3
2
37.
Which of the following equations are correctly balanced?
a)

12CO2 +H2O --> C6H12O6 + O2

b)

CO2 + 9H2O --> C6H12O6 + O2

c)

CO2 + H2O --> 3C6H12O6 + O2

d)

6CO2 + 6H2O --> C6H12O6 + 6O2

38.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words
4
3
2
1
0
39.

What is the correct coefficient for Fe in the balanced equation below?

__Fe + 3O2 → 2Fe2O3

a)

4

b)

3

c)

1

d)

2

40.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)

2

b)

4

c)

6

d)

8

41.
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

42.
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

43.
 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

44.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
45.

Determine the mass of lithium hydroxide produced when 0.38 grams of lithium nitride reacts with water according to the following unbalanced chemical equation: Li3N (s) + H2O (l) → NH3 (g) + LiOH (aq)

(a)   g LiOH

46.

What mass of sodium chloride is produced when chlorine gas reacts with 0.29 grams of sodium iodide? The unbalanced equation is given below: NaI (s) + Cl2 (g) → NaCl (s) + I2 (g)

(a)   g NaCl

47.

Determine the mass of carbon dioxide produced when 0.85 grams of butane (C4H10) reacts with oxygen according to the following balanced chemical equation: 2 C4H10 (l) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g)

4 lines
48.

Determine the mass of calcium hydroxide produced when calcium carbide (CaC2) reacts with 0.64 grams of water according to the following balanced chemical equation: CaC2 (s) + 2 H2O (l) → Ca(OH)2 (aq) + C2H2 (g)

4 lines
49.

Ionic: MgS

a)

Magnesium sulfide

b)

Monomagnesium monosulfide

c)

Magnesium monosulfide

50.

Ionic: Li2O

a)

Dilithium oxideDilithium oxide

b)

Lithium oxide

c)

Lithium dioxide

51.

Ionic: Na2S

a)

Disodium sulfide

Disodium sulfide

b)

Sodium sulfide

c)

Sodium monosulfide

52.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
53.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
54.
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
55.
Li2CO3
a)
Ionic
b)
Covalent
c)
Polyatomic
56.

How many atoms total are in NaOH?

a)

1

b)

2

c)

3

d)

4

57.

How many atoms total are in AlPO4?

a)

4

b)

5

c)

6

d)

7

58.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
59.
What is the formula for iron(II) carbonate?
a)
Fe2CO3
b)
FeCO3
c)
Fe2CO2
d)
FeCO4
60.
Name this compound: 
Ca2CO3
a)
Calcium carbon oxide
b)
Calcium (II) carbonate
c)
Calcium carbonate
d)
Carbonate (I) calcide
61.
What is the formula for copper (II) hydroxide?
a)
CuOH
b)
Cu(OH)2
c)
Cu2OH
d)
Cu2O
62.
Ionic Compounds HAVE a positive (+) or negative (-) charge 
a)
True
b)
False
c)
Que onda, Hagerman? 
d)
What was that now? 
63.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
64.
(NO3) - 
a)
Ionic
b)
Covalent
c)
Polyatomic Ion
d)
Metallic 
65.
The octet rule means that all valence shells want to have the number...... 
a)
1
b)
9
c)
8
d)
16
66.
All atoms/elements bond in order to ....
a)
Have a full valence shell
b)
Give away electrons or take electrons
c)
Only share electrons
d)
To create electrical currents for human use 
67.
Why does NaCl have different charges? 
a)
The metal gives away an electron to the nonmetal
b)
The metal takes the electron from the nonmetal
c)
The metal and the nonmetal equally share electrons
d)
The nonmetal gives away its electrons to the metal 
68.

Covalent: What is the name of N2O3

a)

Nitrogen trioxide

b)

Dinitrogen oxide

c)

Dinitrogen trioxide

d)

Nitrogen oxide

69.

Covalent: What is the name of C3Cl8 ?

a)

Carbon octachloride

b)

Tricarbon octachloride

c)

Carbon trichloride

d)

Octacarbon trichloride

70.

Covalent: What is the chemical formula for Nitrogen triiodide?

a)

NI

b)

N3I

c)

NI3

d)

None of these

71.

Covalent: What is the chemical formula for CP ?

a)

Carbon phosphide

b)

Monocarbon phosphide

c)

Carbon monophosphide

d)

none of the above

72.

Ionic: Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

73.

Ionic: MgS

a)

Magnesium sulfide

b)

Monomagnesium monosulfide

c)

Magnesium monosulfide

74.
Ca+2, O-2
a)
CaO
b)
OCa
c)
Ca-2O+2
d)
Ca2O2
75.
Ca+2P-3
a)
PCa
b)
P2Ca3
c)
CaP
d)
Ca3P2
76.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
77.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
78.
What is the name of NH4Cl?
a)
nitrogen tetrahydrogen chloride
b)
ammonium chlorine
c)
ammonium chloride
d)
ammonium chlorate
79.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
80.
What's the name of the compound NH4NO3 ?
a)
nitrogen hydrogen oxygen
b)
ammonium nitrite
c)
nitrogenous water
d)
ammonium nitrate
81.

An ionic compound is formed between

a)

Metal anion(s) and non-metal cation(s)

b)

Two or more metal atoms

c)

Metal cation(s) and non-metal anion(s)

d)

Two or more non-metal atoms

82.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
83.

Ionic: LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

84.

Which compound naming uses prefixes?

a)

Ionic

b)

Covalent

c)

Ionic and covalent both do

d)

Neither Ionic or covalent do

85.

How do the following two elements bond together?

Al3+ O2- (Hint: How many do I need of each to get a charge of zero?)

a)

AlO

b)

Al2O3

c)

Al3O6

d)

Al3O2

86.

Use the following balanced equation: 2C2H6 + 7O2 ---> 4CO2 + 6H2O

If 15 g of C2H6 react with 45 g of O2, how many grams of water will be produced?

a)

22 g H2O

b)

23 g H2O

c)

27 g H2O

d)

28 g H2O

87.
2NaClO3 (s) → 2NaCl (s) + 3O2 (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
88.
 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
89.

What is the mass of 0.75 moles of (NH4)3PO4?

(a)  

90.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
91.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol

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