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[CHEM] Spring Midterm Review

Total questions: 64

Worksheet time: 3hrs 14mins

Name
Class
Date
1.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
2.
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
3.
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)
124 g O2
4.
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
5.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
6.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
7.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
8.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
9.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
10.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
11.
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
12.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO 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
13.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
14.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
15.

How many zinc(II) atoms are in 65.4 grams of zinc (Zn). (Hint: Look at the periodic table for the Molecular Weight of Zinc. Remember that Grams = MW x Moles)

a)

10

b)

4,277.2

c)

6.02x1023

d)

130.8

16.

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

17.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
18.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
19.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
20.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
21.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
22.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
23.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
c)
C = 92.2%
H = 7.8%
d)
C = 71.9%
H = 28.1%
24.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
25.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
26.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
27.

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

28.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements so that you can give the correct name of the compound formed.

a)

Sulfur monoxide

b)

Sulfur dioxide

c)

Sulfur trioxide

d)

Sulfur tetroxide

29.

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

30.

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

31.
What is the molecular formula for a compound with the empirical formula: CaCl2  and a molecular mass of 330g.
a)
Ca2Cl4
b)
Ca3Cl6
c)
Ca3Cl9
d)
Ca3Cl5
32.

If a chemist calculates the maximum amount of product that could be obtained from a chemical reaction, he or she is calculating the

a)

Theoretical yield

b)

Mole ratio

c)

Actual yield

d)

Percentage yield

33.

What is the measured amount of a product obtained from a chemical reaction?

a)

Mole ratio

b)

Theoretical yield

c)

Percentage yield

d)

Actual yield

34.

In a lab, a scientist calculated that 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)

82.1%

b)

0.82%

c)

10.1%

d)

122%

35.

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%

36.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
37.

ionic compounds get separated into ions in solution through which process

a)

solution

b)

homogeneous solution

c)

dissociation

d)

dissolving

38.

Which end of the water molecule would surround a Cl- ion in a solution

a)

the Oxygen end

b)

the Hydrogen end

c)

neither end

d)

they don't surround the ion

39.

When water molecules completely surround ions or covalent molecules, they form what around them to keep them apart?

a)

hydration shells

b)

a polar bond

c)

an invisible force field

d)

a hydrogen bond

40.

How would you increase the amount of Carbon dioxide dissolved in a bottle of soda?

a)

increase the pressure

b)

heat up the solution

c)

shake up the bottle

41.

How would you increase the amount of carbon dioxide in a bottle of soda to get the maximum amount of CO2 into the liquid?

a)

lower the temperature of the solvent

b)

lower the temperature of the gas

c)

increase the pressure of the gas/solute container

d)

all of these

42.

____________ is the process whereby particles of a solvent completely surround the particles of a solute, disperse them throughout the solvent particles, and hold them in solution.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

43.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

44.

Which of the following ONLY has the effect on the solubility of 'gas'?

a)

Pressure

b)

Temperature

c)

Molarity

d)

Volume

45.

Which one of the following should be increased in order to increase the solubility of a gas?

a)

Temperature

b)

Pressure

46.

amount of solute in a given amount of solvent

a)

concentration

b)

saturated

c)

solution

d)

suspension

47.

any solution that can dissolve more solute at a given temperature

a)

saturated solution

b)

unsaturated solution

c)

supersaturated solution

d)

suspension

48.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

49.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

50.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

51.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

52.
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 
53.
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
54.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
55.

What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?

a)

0.014 %

b)

1.4 %

c)

0.13%

56.

What mass of solute is needed to make 100.0 g of a 3.4% solution?

a)

3.4 g

b)

34 g

c)

2941 g

d)

0.34 g

57.

What is the percent by mass of a solution made by dissolving 10.0 g of NaCl into 180.0 g of water?

a)

5.26 %

b)

5.56 %

c)

180.0 %

d)

20.0 %

58.

What is the percent concentration of sugar in pink lemonade if 28.0 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

11.8 %

59.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

a)

1.6 M

b)

0.63 M

c)

10 M

d)

2.6 M

60.

Sodium chloride (NaCl) and sucrose (C12H22O11) both dissolve in water. Which solution is able to conduct electricity?

a)

sucrose because it is a covalent molecule and nonelectrolyte

b)

sucrose because it is an ionic compound and electrolyte

c)

sodium chloride because it is an ionic compound and electrolyte

d)

sodium chloride because it is a covalent molecule and nonelectrolyte

61.

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

62.
When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
63.

You dissolve 6.00 g of NH4Cl at 70 degrees Celsius. How many more grams will you need to add in order for it to be saturated?

a)

1.00 g more

b)

0.25 g more

c)

0.50 g more

d)

2.00 g more

64.

You dissolve 3.00 g of KNO3 at 45 degrees Celsius. How many more grams will you need to add in order for it to be saturated?

a)

1.00 g more

b)

0.25 g more

c)

0.50 g more

d)

2.00 g more

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