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G9 Chemistry Final Exam Review Part 3

Total questions: 60

Worksheet time: 5hrs 43mins

Name
Class
Date
1.

Find the molar mass of CaCO3CaCO_3   

a)

100.09g

b)

100g

c)

100.2g

d)

101g

2.

Find the number of moles in 75 grams of NaHCO3NaHCO_3   

a)

89mol

b)

0.90mol

c)

0.89mol

d)

84mol

3.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
4.

What units are used for molar mass?

a)

gramsmole\frac{grams}{mole}  

b)

molesatom\frac{moles}{atom}  

c)

AMUAMU  

d)

degrees Fahrenheit

5.

How many moles of oxygen atoms are in 31.998 grams of oxygen?

To solve this problem you should...

a)

multiply by 1 mole6.022x1023\frac{1\ mole}{6.022x10^{23}}  

b)

multiply by  1 mole15.999 g\ \frac{1\ mole}{15.999\ g}  

c)

multiply by 6.022x10231 mole\frac{6.022x10^{23}}{1\ mole}  

d)

multiply by 15.999 g1 mole\frac{15.999\ g}{1\ mole}  

6.

How many moles of oxygen atoms are in 3.011 x 10^23 atoms of oxygen?

To solve this problem you should...

a)

multiply by 1 mole6.022x1023\frac{1\ mole}{6.022x10^{23}}  

b)

multiply by  1 mole15.999 g\ \frac{1\ mole}{15.999\ g}  

c)

multiply by 6.022x10231 mole\frac{6.022x10^{23}}{1\ mole}  

d)

multiply by 15.999 g1 mole\frac{15.999\ g}{1\ mole}  

7.
The molar mass of an element is the mass of one ____ of the element.
a)
atom
b)
molecule
c)
mole
d)
gram
8.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
9.
How many moles are in 4.5x1024 particles?
a)

7.47 particles

b)

7.47mol

c)
2.71x1047 mol
d)
2.71x1047 particles
10.

85.0 g of NaOH is equal to how many moles?

a)

3400 moles

b)

45 moles

c)

0.47 moles

d)

2.1 moles

11.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
12.
What is the closets molar mass of B2(CO3)3?
a)
81.632 g/mol
b)
94.842 g/mol
c)
38.822 g/mol
d)
201.648 g/mol
13.
Fluorine is diatomic.  What is the closets molar mass of fluorine gas?
a)
18.998 g/mol
b)
37.996 g/mol
c)
9 g/mol
d)
18 g/mol
14.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
15.
What is the closest percent composition by mass of sulfur in the compound MgSO4 (MgSO4 formula mass = 120 g/mol)?
a)
18%
b)
27%
c)
46%
d)
53%
16.
In which compound is the percent composition by mass of Cl closest to 42%?
a)
HClO (gram formula mass = 52 g/mol)
b)
HClO2 (gram formula mass = 68 g/mol)
c)
HClO3 (gram formula mass = 84 g/mol)
d)
HClO4 (gram formula mass = 100 g/mol)
17.
What percent of Zn3(PO4)2 is zinc?
a)
33.15%
b)
16.04%
c)
50.81%
d)
19.68%
18.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
19.
Which list of number for the atoms in Mg(NO3)2 is right?
a)
Mg = 1, N = 6,  O =  6
b)
Mg = 1, N = 6,  O =  2
c)
Mg = 2, N = 2,  O =  6
d)
Mg = 1, N = 2,  O =  6
20.
Find the percent composition of compound that contains 1.51 g of chromium, 1.13 g of potassium, and 1.62 g of oxygen.  The total mass of the sample is 4.26 g.
a)
Cr = 26.5%; K = 38.0%; O = 35.4%
b)
Cr = 38.0%; K = 35.4%; O = 26.5%
c)
Cr = 38.0%; K = 26.5%; O = 35.4%
d)
Cr = 35.4%; K = 26.5%; O = 38.0%
21.
What is the percent composition of a compound that contains 40.8 g carbon and 54.4 g oxygen?
a)
42.9 % carbon; 57.1% oxygen
b)
57.1 % carbon; 42.9 % oxygen
c)
40.8 % carbon; 54.4 % oxygen
d)
54.4 % carbon; 40.8% oxygen
22.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
23.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
24.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
25.
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
26.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
27.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
28.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
29.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
30.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
31.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
32.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
33.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K
34.
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 
35.
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
36.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
37.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
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 (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
39.
100 degrees Celsius is equal to _______ Kelvin. 
a)
0 K
b)
273 K
c)
173 K
d)
373 K
40.

What term do we use to describe a less concentrated solution?

a)

Dilute

b)

Volume

c)

Aqueous

d)

Solvent

41.

Which of the solutions above is the most dilute

a)

A

b)

C

c)

E

d)

They are all the same concentration

42.

Which solution is more concentrated?

Solution 1:

5 L of water

100 g of salt


Solution 2:

5 L of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

43.

If 43.0 g of sodium chloride is dissolved in 500 g of Acetic acid, what is the percent by mass of NaCl?

a)

7.90 %

b)

8.60 %

c)

11.6 %

d)

92.1 %

44.

If 248 ml of acetone is mixed with 562 ml of water, what is the percent by volume of acetone?

a)

69.4 %

b)

44.0 %

c)

30.6 %

d)

2.23 %

45.

What is the molar mass of Fel2?

a)

55.85 g/mol

b)

126.90 g/mol

c)

239.65 g/mol

d)

309.65 g/mol

46.

What is the molar mass of Ca(OH)2?

a)

58.10 g/mol

b)

73.09 g/mol

c)

74.10 g/mol

d)

114.18 g/mol

47.

How many mol of solute are dissolved in 125.0 dm3dm^3 of 5.00M NaCl?

a)

0.625 mol NaCl

b)

36.52 mol NaCl

c)

36.5 mol NaCl

d)

0.625 mol NaCl

48.

What is the percent by mass of a sugar solution where 10 grams of sugar is added to 100 grams of water?

a)

.10%

b)

0.091%

c)

9.1%

49.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

50.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
51.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
52.
An 8 g sample of a compound is found to be 3.766 g Aluminum & 4.234 g Oxygen.  What is it's empirical formula?
4 lines
53.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

54.

What is the number of atoms in 0.0100 mol of NH3?

(The Avogadro constant NA = 6.022 × 1023 particles/mol)

a)

6.02 × 1025

b)

1.20 × 1023

c)

1.81 × 1022

d)

2.41 × 1022

55.

How many molecules of iodine are in 0.1 mole of iodine, I2?

a)

25.38g

b)

6.02 x 1022

c)

1.204 x 1024

d)

6.02 x 1023

56.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
57.

Which of these contains the most molecules?

a)

0.0311 kg of carbon dioxide, CO2

b)

29.6 g of carbon monoxide, CO

c)

2.22 × 104 mg of oxygen, O2

d)

13.3 g of ozone, O3

58.

How many moles of carbon atoms are there in 5g of carbon?

a)

60 moles

b)

17 moles

c)

0.42 moles

d)

7 moles

59.

How many moles are there in 12.7g of CaF2?

a)

0.20 moles

b)

1,000.76 moles

c)

6.14 moles

d)

0.16 moles

60.

How many atoms of copper in 65.0 g of copper(II) chloride?

a)

2.91 ×1023 atoms2.91\ \times10^{23}\ atoms  

b)

3.95 ×1023 atoms3.95\ \times10^{23}\ atoms  

c)

  5.81×1023 atoms5.81\times10^{23}\ atoms  

d)

  7.90×1023 atoms7.90\times10^{23}\ atoms  

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