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Unit 5 Test Review (Mass Relationships)

Total questions: 50

Worksheet time: 4hrs 6mins

Name
Class
Date
1.

What is the SI base unit of quantity?

a)

Liter

b)

Gram

c)

Mole

d)

Atoms

2.

Which isotope is the mole and amu standards based on?

a)

12C

b)

13C

c)

1H

d)

2H

3.

When reading a chemical equation (e.g. 4Al + 3O2 → 2Al2O3), what type of units should be used when “reading” it?

a)

Volume

b)

Quantity

c)

Mass

d)

Length

4.

Which of the following is not known to be equal to the others?

a)

4.00 grams of Helium

b)

1.00 moles of Nitrogen

c)

6.02 liters of Argon

d)

40.08 grams of Calcium

5.

What is the average atomic mass for an element X the following two isotope masses and relative abundances?

37% at 33.79 amu and 63% at 35.53 amu

a)

34.66 amu

b)

34.89 amu

c)

34.30 amu

d)

35.45 amu

e)

34.59 amu

6.

A one carat diamond contains approximately 0.20 grams of carbon, how many moles of carbon is this?

a)

0.017 mol

b)

1.2 mol

c)

1.0 x 102210^{22} mol

d)

2.4 mol

e)

0.033 mol

7.

How many moles are present in 6.7 grams of AlCl3?

a)

0.050 moles

b)

0.150 moles

c)

0.081 moles

d)

0.025 moles

e)

0.30 moles

8.

A container possesses 6.28 moles of Neon. How many grams of Neon (Ne) are present?

a)

320 g

b)

127 g

c)

0.123 g

d)

0.311 g

e)

450 g

9.

A decomposition reaction produces 3.56 moles of sulfur. How many grams of Sulfur is this?

a)

9.02 g

b)

2.14 x 10^24 g

c)

0.111 g

d)

5.91 x 10^{-24} g

e)

114 g

10.

What scientific law is being obeyed when a chemical equation is balanced?

a)

Law of Conservation of Mass

b)

Avogadro's Law

c)

Law of Definite Proportions

d)

Kepler's Law

11.

How many atoms of Fe are found in 4.23 grams?

a)

2.55 x 10^24

b)

1.42 x 10^26

c)

1.26 x 10^21

d)

4.63 x 10^22

e)

4.56 x 10^22

12.

100 grams of Hydrogen Iodide & 100 grams of Hydrogen Fluoride will possess the same number of molecules.

a)

True

b)

False

13.

What is the molar mass of CaCl2?

a)

110.98 g

b)

40.08 g

c)

58.44 g

d)

74.55 g

14.

While Carbon-12 has a mass of 12 amu, Magnesium-24 does not have an exact mass of 24 amu due to the mass defect.

a)

True

b)

False

15.

The Mass Spectrometer uses a strong LASER to separate particles by their varying mass.

a)

True

b)

False

16.

A molecule has an empirical formula of C1H2 and a molar mass 70 grams per mole. What is the molecular formula?

a)

C4H22

b)

C6H12

c)

C3H6

d)

C5H10

17.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
18.

How many atoms can be found in a 5,750 gram copper pipe?

a)

3.46 x 10^27 atoms

b)

545 atoms

c)

90.6 atoms

d)

5.45 x 10^25 atoms

e)

2.20 x 10^29 atoms

19.

The atomic mass listed on the periodic table accounts for both the mass defect and the average atomic mass of the various existing isotopes.

a)

True

b)

False

20.

What numerical quantity represented in the grouping number known as the mole?

a)

2.18 x 10^18

b)

6.63 x 10^34

c)

6.02 x 10^23

d)

3.00 x 10^8

e)

1.66 x 10^24

21.

What is the numerical value of 1 mole referred to as?

a)

Lavoisier’s number

b)

Perrin’s number

c)

Avogadro’s number

d)

Mole number

22.

What is the molar mass of Pentose (C5H10O5)?

a)

20.0 g

b)

96.0 g

c)

180.0 g

d)

145.0 g

e)

150.0 g

23.

What is the molar mass of Sr(NO3)2?

a)

117.6 g

b)

149.6 g

c)

195.6 g

d)

211.6 g

e)

100.0 g

24.

How many atoms of hydrogen are in 89.6 grams ammonia (NH3)?

a)

3.17 x 10^24 atoms

b)

6.02 x 10^22 atoms

c)

1.57 x 10^22 atoms

d)

9.52 x 10^24 atoms

e)

1.06 x 10^24 atoms

25.

How many hydrogen atoms are found in 97.6 grams of C2H6?

a)

1.96 x 10^24

b)

1.18 x 10^25

c)

9.79 x 10^24

d)

7.05 x 10^27

e)

5.88 x 10^25

26.

Francis Aston’s Mass spectrometer uses a strong magnetic field to deflect particles to separate them by their varying mass.

a)

True

b)

False

27.

The empirical formula reports the exact number of atoms present in a compound.

a)

True

b)

False

28.

What is the percent composition of Aluminum in Galaxite: Mn(AlO2)2?

a)

15.6 %

b)

5.4 %

c)

10.8 %

d)

31.2 %

e)

172.9 %

29.

A molecule has the mass percentage composition of 21.0% Si, 70.93% Cl, and 8.00% O. What is the empirical formula of this compound (SiₓClᵧO𝓏)?

a)

Si₁Cl₂O₁

b)

Si₃Cl₄O₁

c)

Si₃Cl₉O₁

d)

Si₂Cl₄O₁

e)

Si3Cl8O2

30.

A compound has the empirical formula of C₄H₅N₂O. The molar mass has been determined to be 194 grams. Determine the molecular formula of this compound.

a)

C₄H₅N₂O

b)

C₁₀H₁₆N₆O₃

c)

C₁₀H₁₆N₃O₁

d)

C₂₀H₁₂N₁₂O₆

e)

C₈H₁₀N₄O₂

31.

What is the coefficient for H₂O when the following chemical equation is balanced? ___Al(OH)₃ + ___H₂SO₄ → ___H₂O + ___Al₂(SO₄)₃

a)

6

b)

4

c)

1

d)

5

e)

7

32.

What term describes the quantitative relationship between reactants and products in a chemical reaction?

a)

Spectrometry

b)

Stochioscopy

c)

Stoichiometry

d)

Spectroscopy

33.

How many grams of KCl (74.55 g/mol) are made when 132.5 grams of K₂CrO₄ (194.19 g/mol) react? 3 K₂CrO₄ + 2 BiCl₃ → 6 KCl + Bi₂(CrO₄)₃

a)

101.7 g

b)

66.25 g

c)

305.2 g

d)

25.43 g

e)

265.0 g

34.

What is the coefficient in front of O₂ when the following chemical equation is balanced? ___C₄H₄O₂ + ___O₂ → ___CO₂ + ___H₂O

a)

2

b)

1

c)

5

d)

4

e)

3

35.

If you have 82.21 grams of NO2, how many molecules do you have?

Pick the correct setup.

a)

82.21 g ×1 mol46.01 g×1 mol6.02x1023 molecules82.21\ g\ \times\frac{1\ mol}{46.01\ g}\times\frac{1\ mol}{6.02x10^{23}\ molecules}  

b)

82.21 g ×1 mol46.01 g×6.02x1023 molecules1 mol82.21\ g\ \times\frac{1\ mol}{46.01\ g}\times\frac{6.02x10^{23}\ molecules}{1\ mol}  

c)

82.21 g ×6.02x1023 molecules1 mol82.21\ g\ \times\frac{6.02x10^{23}\ molecules}{1\ mol}  

d)

82.21 g ×1 mol46.01 g82.21\ g\ \times\frac{1\ mol}{46.01\ g}  

36.

Balance the below chemical reaction. What is the coefficient in front of O2 when balanced?

CH4 + O2 → CO2 + H2O

a)

2

b)

1

c)

3

d)

4

37.

A chemical reaction is performed and theoretically expected to make 48.6 grams of product. However only 31.5 grams is actually collected. What is the percent yield of the reaction?

a)

31.5%

b)

15.4%

c)

35.1%

d)

64.8%

e)

1.54%

38.

Which statement about reactions is not supported by the Law of Conservation of Mass?

a)

A) The number of atoms on the reactant side is going to be the equal to the atoms on the product side of a reaction.

b)

B) The speed of a chemical reaction will increase as the mass of reactants is increased.

39.

If the reactants are in the correct stoichiometric equivalent amounts, the total mass of reactants is going to be equal to the total mass of products.

a)

True

b)

False

40.

Fill in the blank: A chemical reaction only rearranges the atoms of the reactants, but does not create or ______ any atoms.

a)

destroy

b)

multiply

c)

color

d)

charge

41.

Which law states that matter is neither created nor destroyed in a chemical reaction?

a)

Law of Conservation of Mass

b)

Law of Multiple Proportions

c)

Boyle's Law

d)

Charles's Law

42.

Which instrument is commonly used to determine the relative abundance of isotopes in a sample?

a)

Thermometer

b)

Barometer

c)

Voltmeter

d)

Mass spectrometer

43.

Which instrument is commonly used to determine the relative abundance of isotopes in a sample using magnetic fields?

a)

Thermometer

b)

Barometer

c)

Voltmeter

d)

Mass spectrometer

44.

Which of the models of a chemical reaction best represents the Law of Conservation of Mass?

a)

A

b)

B

c)

C

d)

D

45.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
46.

82.3 g of Mg reacts with 57.9 g of N2 to form Mg3N2.

What is the theoretical yield?

(hint: 2 calculations are necessary)

a)

114 g

b)

82.3 g

c)

57.9 g

d)

140.2 g

e)

209 g

47.
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
48.

What is the limiting reactant when 37 g NaCl & 18 g Al are combined in the following reaction to generate sodium metal (Na)? 3NaCl + Al → AlCl3 + 3Na

a)

NaCl

b)

Na

c)

Al

d)

O2

e)

AlCl3

49.

What is the limiting reactant when 50 grams of Hydrogen gas (2 g/mol) and 50 grams of fluorine gas (38 g/mol) are reacted to form HF (20 g/mol)? H2 + F2 → 2HF

a)

H2

b)

F2

c)

HF

50.

Which of the following statements is false?

a)

Ionic compounds formulas are always the same as their empirical formulas.

b)

10 grams of Helium will possess more atoms than 10 grams of Neon.

c)

Percent composition is an extensive property.

d)

1 mole is also known as Avogadro's number

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