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Kennedy--Interim #2 Review (solutions and stoichiometry)

Total questions: 74

Worksheet time: 6hrs 10mins

Name
Class
Date
1.

Solid solutes dissolve quicker in _________ water.

a)

cold

b)

warm

2.

Gas solutes dissolve better in _________ water.

a)

cold

b)

warm

3.

The substance being dissolved in a solution is the?

a)

solution

b)

solute

c)

solvent

d)

mixture

4.

The substance in which a solute is dissolved is a?

a)

solution

b)

solvent

c)

alloy

d)

mixture

5.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
6.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
7.

If I dissolve sugar in water, what is the solvent?

a)

Sugar

b)

There is no solvent

c)

Oxygen

d)

Water

8.

At 80'C, KBr's solubility is:

a)

100g

b)

90g

c)

80g

d)

0g

9.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

10.

Which of these solutes is a gas and how do you know?

a)

Yb2(SO4)3 because it has a negative slope

b)

NaCl because it has a zero slope

c)

KNO3 because it has a positive slope

11.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

60 g

d)

33 g

12.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
13.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
14.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
15.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
16.
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
17.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
18.
Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.
a)
0.750 M
b)
99 M
c)
1.3 M
d)
2.0 M
19.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
20.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
21.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
22.

What distinguishes the boiling point from the melting point of a substance?

a)

The boiling point is the temperature at which a liquid turns into a gas, while the melting point is the temperature at which a solid turns into a liquid.

b)

The boiling point is the temperature at which a solid turns into a gas, while the melting point is the temperature at which a gas turns into a liquid.

c)

The boiling point is lower than the melting point.

d)

The boiling point and melting point are the same for all substances.

23.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
24.
CO2
a)
Ionic 
b)
Covalent
25.
CaCl2
a)
Ionic 
b)
Covalent
26.
NH3
a)
Ionic 
b)
Covalent
27.
MgO
a)
Ionic 
b)
Covalent
28.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
29.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
30.

Which one of the following statements is true about solutions that conduct electricity?

a)

The salt solution conducts electricity because ionic compounds dissociate into ions when dissolved in water.

b)

The sugar solution conducts electricity because covalent compounds solvate and the molecule stays intact when dissolved in water.

c)

The pure water conducts electricity really well on its own.

31.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

32.

Calculate the molar mass of CO2.

a)

14 g/mol

b)

28 g/mol

c)

36 g/mol

d)

44 g/mol

33.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

34.

Avogadro's number of atoms is equal to one_____ of atoms.

a)
kilogram
b)
gram
c)
kelvin
d)
mole
35.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction. 
d)
Mechanism involved in the reaction. 
36.
Where do you look to calculate the molar mass?
a)
avogadros number
b)
periodic table 
37.
Find the percent composition of N2S2.
a)
N: 69.6%  S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
38.
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
39.
Find the mass in grams of 0.75 moles of magnesium (Mg).
a)
32 grams
b)
18 grams
c)
2.21 x 10 ^23 grams
40.
3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe
What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
41.
H2+Cl2-->2HCl
How many moles of Cl2 are needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
42.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
43.

Determine the volume, in liters, of 1.2 mole SO2 gas at STP.

a)

13 L

b)

26 L

c)

6.5 L

44.

Match the following units to their correct category.

a)

Grams

1.

Mass

b)

Liters at STP

2.

Volume

c)

Units, Atomes, Molecules

3.

Particles

45.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

46.
How are the mole and atomic masses of elements related?  
a)
The atomic mass of any substance is always equal to 1 mole of that substance 
b)
The atomic mass added up with itself by 6.02 x 1023 equals the amount of atoms
c)
The atomic mass is the amount of protons plus number of atoms
d)
Atoms combined make up molecules, which are the measurement of atomic masses 
47.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)

44.01 moles

b)

1421.52 moles

c)

32.3 moles

d)

0.73 moles

48.

What is the mass of 2.50 mole of oxygen gas O2?

a)

40 g

b)

80 g

c)

16 g

d)

32 g

49.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

50.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

51.
Question Image

Match the following...

a)

You convert moles to grams by...

1.

multiplying by the molar mass

b)

You convert liters to moles by...

2.

dividing by 22.4L

c)

You convert moles to particles by...

3.

multiplying my avagadro's constant

d)

You convert grams to moles by...

4.

dividing by the molar mass

e)

You convert moles to liters by...

5.

multiplying by 22.4L

52.

What is the percent composition of oxygen in MgO?

a)

20%

b)

40%

c)

50%

d)

60%

53.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

54.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
55.
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%
56.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
57.
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
58.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)

5.3 g

b)
2.6 g
c)
690 g
d)
45 g
59.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)

125 g O2

60.

Which of the following is necessary to switch from one substance to another in a stoichiometry problem?

a)

Molar Mass

b)

Molar Ratio

c)

Periodic Table

d)

Specific Heat

61.

Put the following steps in the correct order to solve the stoichiometry problem.

a)

10.1 grams HCl/1

b)

1 mol HCl/36.460 grams HCl

c)

2 mol Cl/1 mol HCl

d)

35.453 grams Cl/1 mol Cl

e)

19.6 grams Cl/1

1)
2)
3)
4)
5)
62.

Balance the following equation with the correct coefficients:

___ SnO₂ + ___ H₂ → ___ Sn + ___ H₂O

a)

1, 2, 1, 2

b)

2, 1, 1, 2

c)

1, 1, 1, 1

d)

2, 2, 3, 2

63.

Balance the following equation with the correct coefficients:

KOH + H₃PO₄ → K₃PO₄ + H₂O

a)

3, 1, 1, 3

b)

2, 1, 3, 2

c)

1, 1, 1, 1

d)

2, 2, 3, 2

64.

Using the diagram, determine the limiting reactant, the product formed is water.

a)

oxygen

b)

hydrogen

c)

none of the reactant are limiting

d)

both hydrogen and oxygen

65.

It refers to the substance(s) that are considered to be "ingredients" of a chemical reaction.

a)

reactants

b)

products

c)

catalysts

d)

enhancers

66.

The ____ in a balanced chemical reactions gives the MOLE RATIO used in stoichiometry problems.

a)

coefficients

b)

reactants

c)

subscripts

d)

products

67.

In this image, what is the information to the right of the arrow (in black) is called the_______.

a)

Product

b)

Reactant

c)

Chemical Subscript

d)

Yield

68.

Hydrogen and oxygen molecules combine to form water molecules as shown in the reaction below. Given the molecules provided, which of the following is true about the products of this reaction? 

a)

2 H2O molecules are produced, O2 is the limiting reactant

b)

4 H2O molecules are produced, H2 is the limiting reactant

c)

4 H2O molecules are produced, O2 is the limiting reactant

d)

6 H2O molecules are produced, H2 is the limiting reactant

69.

Which of the following describes an excess reactant?

a)

The reactant that is not completely consumed during a reaction

b)

None of this reactant is left over after the reaction take place

c)

The reactant that is completely consumed during the reaction

70.

Which of the following describes a limiting reactant?

a)

The reactant that is not completely consumed during a reaction

b)

The reactant that is completely consumed during the reaction

c)

Some of this reaction is left over after the reaction

71.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
72.

Molecular Formula = C2F6

Choose the correct empirical formula.

a)

CF

b)

C2F6

c)

C3F

d)

CF3

73.

Empirical Formula = CF2

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

74.

The empirical formula of a substance is CH2O. The molar mass is 180g/mol. What is the molecular formula?

a)

CH2O

b)

C3H6O3

c)

C6H12O6

d)

C12H6O12

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