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Chemistry 1 Second Semester Study Questions

Total questions: 61

Worksheet time: 5hrs 5mins

Name
Class
Date
1.

When there is an unequal sharing of electrons in a bond, the bond is said to be __

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

2.

The greater the difference in the electronegativities of the bonding atoms

a)

the more nonpolar the bond

b)

the more polar the bond

c)

the more equal the sharing of electrons

d)

the more nonpolar the bond and the more equal the sharing of electrons

e)

the more polar the bond and the more equal the sharing of electrons

3.

A molecule of CH4 is

a)

asymmetrical and polar

b)

asymmetrical and nonpolar

c)

symmetrical and polar

d)

symmetrical and nonpolar

4.

A bond between C and F would be

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

5.

Which of the following pairs of molecules and their shape, and bond angle is correct?

a)

CF4 - tetrahedral - 109.5

b)

BeBr2 - linear - 120

c)

H2O - tetrahedral - 104.5

d)

NH3 - trigonal pyramidal - 109.5

e)

PCl3 - trigonal pyramidal - 120

6.

Which of the following molecules has a trigonal pyramidal molecular shape?

a)

CH4

b)

H2O

c)

CO2

d)

NH3

e)

BF3

7.

What kind of hybridization is occurring in the XA4 molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

e)

spd2

8.

The molar mass of (NH4)2S is closest to:

a)

50 g/mol

b)

82 g/mol

c)

68 g/mol

d)

100 g/mol

9.

How many atoms are in 12 molecules of glucose, C6H12O6?

a)

24

b)

2160

c)

288

d)

7.22 x 1024

10.

Calculate the number of atoms in 4.0 x 10-5 g of aluminum.

a)

8.9 x 1017

b)

4.6 x 1019

c)

6.5 x 1020

d)

3.8 x 1023

11.

A compound consists of the following elements by weight percent:


carbon - 40.0%

oxygen - 53.3%

hydrogen - 6.7%


The ratio of carbon : oxygen : hydrogen in the empirical formula is

a)

1:2:1

b)

1:1:2

c)

1:1:1

d)

2:1:2

12.

Which of the following samples contains the smallest number of atoms?

a)

1 g H2

b)

1 g O2

c)

1 g O3

d)

1 g Cl2

13.

An organic compound which has the empirical formula CHO has a molar mass of 232.

Its molecular formula is:

a)

CHO

b)

C2H2O2

c)

C4H4O4

d)

C8H8O8

14.

What is the percent nitrogen (by mass) in ammonium carbonate, (NH4)2CO3?

a)

14.53%

b)

27.83%

c)

29.16%

d)

33.34%

15.

Of the following, the only empirical formula is

a)

N2F2

b)

N2F4

c)

H2C2

d)

HNF2

16.

When CaSO4 ·y H2O is heated, all of the water is driven off. If 34.0 g of CaSO4 [molar mass = 136] is formed from 43.0 g of CaSO4 ·y H2O, what is the value of y?

a)

1

b)

3

c)

2

d)

4

17.

What is the mass of one molecule of octane, C8H18?

a)

114 g

b)

1.89 x 10-22 g

c)

1.10 x 10-22 g

d)

4.32 x 10-23 g

18.

Balance the following equation:

___NH3 + ___O2 → ___NO2 + ___H2O

The balanced equation shows that 1.00 mole of NH3 requires ___ mole(s) of O2.

a)

0.57

b)

1.25

c)

1.33

d)

1.75

19.

Write a balanced equation for the combustion of acetaldehyde, CH3CHO.

a)

2 CH3CHO + 5 O2 ---> 4 CO2 + 4 H2O

b)

CH3CHO + O2 ---> 4 CO2 + 4 H2O

c)

2 CH3CHO ---> CO2 + 3 H2O

d)

CH3CHO + O2 ---> CO2 + H2O

20.

When properly balanced, the equation indicates that ___mole(s) of O2 are required foreach mole of CH3CHO.

a)

1

b)

2

c)

2.5

d)

3

21.

What is the total mass of products formed when 16 grams of CH4 is burned with excess

oxygen?

a)

80 g

b)

44 g

c)

36 g

d)

32 g

22.

a) 2Fe + O2 --> 2FeO

b) 3Ca(OH)2 + 2H3 PO4 --> Ca3(PO4)2 + 6H2O

c) 2NaCl --> 2Na + Cl2

d) C7H16 + 11O2 --> 7CO2 + 8H2O

e) Fe + CuSO4 --> FeSO4 + Cu

Which of the above reactions is a single replacement?

a)

D

b)

E

c)

C

d)

A

23.

a) 2Fe + O2 --> 2FeO

b) 3Ca(OH)2 + 2H3 PO4 --> Ca3(PO4)2 + 6H2O

c) 2NaCl --> 2Na + Cl2

d) C7H16 + 11O2 --> 7CO2 + 8H2O

e) Fe + CuSO4 --> FeSO4 + Cu

Which of the above reactions is decomposition?

a)

C

b)

B

c)

D

d)

E

24.

a) 2Fe + O2 --> 2FeO

b) 3Ca(OH)2 + 2H3 PO4 --> Ca3(PO4)2 + 6H2O

c) 2NaCl --> 2Na + Cl2

d) C7H16 + 11O2 --> 7CO2 + 8H2O

e) Fe + CuSO4 --> FeSO4 + Cu

Which of the above reactions is combustion?

a)

A

b)

E

c)

B

d)

D

25.

What is (are) the product(s) of the reaction:

Mg(CO3)2 (s) -->

a)

Mg (s) + C (s) + 3 O2 (g)

b)

Mg (s) + C (s) + 6 O2 (g)

c)

Mg-2 (aq) + CO3-2 (aq)

d)

MgO (s) + CO2 (g)

26.

What is (are) the unbalanced products of the following reaction:

CH4 (g) + O2 (g) -->

a)

CO2 (g) + H2O (g)

b)

CH3OH (aq)

c)

CO2 (g) + H2 (g)

d)

CH3OCH3

27.

What type of reaction is shown below, and what is the correct balanced equation?

Magnesium + water --> magnesium hydroxide + hydrogen gas

a)

Single replacement; Mg + 2 H2O --> Mg(OH)2 + H2

b)

Double replacement; Mg2 + 3 H2O --> 2 Mg(OH)2 + H2

c)

Double replacement; Mg2 + 2 H2O --> Mg(OH)2 + H

d)

Single replacement; Mg + H2O --> Mg(OH)2 + H2

28.

What type of reaction is shown below, and what is the correct balanced equation?

copper metal + silver nitrate → silver metal + copper II nitrate

a)

Double replacement; Cu2 + 2 AgNO3 --> 2 Ag2 + Cu(NO3)2

b)

Synthesis; Cu + AgNO3 --> Ag + Cu(NO3)2

c)

Single replacement; Cu + 2 AgNO3 --> 2 Ag + Cu(NO3)2

d)

Single replacement; Cu + 2 AgNO3 --> Ag2 + Cu(NO3)2

29.

Calculate the mass of hydrogen formed when 25 g of aluminum reacts with excess hydrochloric acid.

2 Al + 6 HCl --> 2 AlCl3 + 3 H2

a)

0.41 g

b)

0.92 g

c)

1.2 g

d)

2.8 g

30.

How many grams of the mixed oxide, Fe 3 O 4 , are formed when 6.00 g of O 2 react with Fe according to

3 Fe + 2 O2 → Fe3O4

a)

43.4

b)

86.8

c)

174

d)

21.7

31.

For the reaction:

2MnO 2 + 4KOH + O 2 + Cl 2 →2KMnO 4 + 2KCl + 2H 2 O

There are 100. g of each reactant available. Which reagent is the limiting reagent?

[Molar Masses: MnO 2 =86.9; KOH=56.1; O 2 =32.0; Cl 2 =70.9]

a)

MnO2

b)

KOH

c)

O2

d)

Cl2

32.

How many grams of nitric acid, HNO3, can be prepared from the reaction of 92.0 g of NO2 with 36.0 g H2O?

3NO2 + H2O --> 2HNO3 + NO

a)

64

b)

76

c)

84

d)

116

33.

The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield?

C6H6 + HNO3 --> C6H5NO2 + H2O

a)

100%

b)

27.4%

c)

54.3%

d)

85.6%

34.

How many grams of H2O will be formed when 16.0 g H2 is allowed to react with 16.0 g O2 according to

2 H2 + O2 --> 2 H2O?

a)

180.0 g

b)

144 g

c)

9.00 g

d)

32.0 g

35.

Aluminum reacts with oxygen to produce aluminum oxide.

4 Al (s) + 3 O2 (g) → 2 Al2O3 (s)

If 5.0 moles of Al react with excess O2 , how many moles of Al2O3 can be formed?

a)

1.0 mol

b)

2.0 mol

c)

2.5 mol

d)

5.0 mol

e)

10.0 mol

36.

Sodium carbonate reacts with hydrochloric acid as shown below in an unbalanced chemical equation. What mass of CO2 is produced from the reaction of 2.94 g Na2CO3 with excess HCl?

Na2CO3 (s) + HCl (aq) → NaCl (aq) + CO2 (g) + H2O (l)

a)

1.22 g

b)

2.44 g

c)

2.94 g

d)

5.88 g

e)

7.08 g

37.

Nitric oxide is made from the oxidation of ammonia. How many moles of nitric oxide can be made from the reaction of 3.80 mol NH3 with 5.15 mol O2?

4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)

a)

3.80 mol

b)

4.12 mol

c)

5.15 mol

d)

6.44 mol

e)

8.95 mol

38.

The reaction of 10.0 g H2 (g) with 10.0 g O2 (g) yields 8.43 g H2O (g). What is the percent yield of this reaction?

a)

9.43%

b)

27.3%

c)

42.2%

d)

66.8%

e)

74.9%

39.

A 4.00 M solution of H3PO4 will contain ___g of H3PO4 in 0.250 L of solution.

a)

196 g

b)

98.0 g

c)

49.0 g

d)

24.0 g

e)

12.0 g

40.

How many milliliters of 0.123 M NaOH solution contain 25.0 g of NaOH (molar mass = 40.00 g/mol)?

a)

5.08 mL

b)

50.8 mL

c)

508 mL

d)

625 mL

e)

5080 mL

41.

If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution?

a)

Add 950. mL of water to 50.0 mL of 3.00 M H2SO4

b)

Add 500. mL of water to 500. mL of 0.500 M H2SO4

c)

Add 750 mL of water to 250 mL of 0.375 M H2SO4

d)

Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L

e)

Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L

42.

Carbon dioxide in water is an example of which solute-solvent combination?

a)

gas-liquid

b)

liquid-gas

c)

liquid-liquid

d)

cannot be determined

43.

What is the ion concentration in a 0.12 M solution of BaCl2?

a)

[Ba2+]=0.12 M and [Cl-]= 0.12 M

b)

[Ba2+]=0.12 M and [Cl-]= 0.060 M

c)

[Ba2+]=0.12 M and [Cl-]= 0.24 M

d)

[Ba2+]=0.060 M and [Cl-]= 0.060 M

e)

[Ba+]=0.12 M and [Cl2-]= 0.12 M

44.

How does a gas expand?

a)

Its particles become larger

b)

Collisions become elastic

c)

Its temperature rises

d)

Its particles move farther apart

45.

What happens to the volume of a gas during compression?

a)

The volume increases

b)

The volume decreases

c)

The volume remains constant

d)

It is impossible to tell because all gases are different

46.

A pressure of 700. kPa is equal to ______ mmHg.

a)

40.0 mm Hg

b)

401 mm Hg

c)

1060 mm Hg

d)

5250 mm Hg

47.

Pressure and volume changes at a constant temperature can be calculated using

a)

Boyle's Law

b)

Charles's Law

c)

Kelvin's Law

d)

Dalton's Law

48.

A sample of a gas has a volume of 150 mL when its pressure is 0.947 atm. What will the volume of the gas be at a pressure of 0.987 atm?

a)

140 mL

b)

144 mL

c)

152 mL

d)

156 mL

49.

A sample of gas occupies a volume of 752 mL at 25°C. What volume will the gas occupy if the temperature increases to 50°C?

a)

376 mL

b)

694 mL

c)

815 mL

d)

1500 mL

50.

Calculate the volume of 0.600 moles of a gas at 15.0°C and a pressure of 1.10 atm.

a)

12.9 L

b)

22.4 L

c)

24.6 L

d)

129 L

51.

A 1.00 L sample of a gas has a mass of 1.92 g at STP. What is the molar mass of the gas?

a)

1.92 g/mol

b)

19.2 g/mol

c)

22.4 g/mol

d)

43.0 g/mol

52.

The Ideal Gas Law works the best when the gas is at

a)

high T and low P

b)

low T and low P

c)

low T and high P

d)

high T and high P

53.

The volume and temperature of a gas are

a)

inversely related

b)

directly related

c)

disproportionate to one another

d)

none of these

54.

Calculate the pH of a solution in which

[OH-] = 2.50 × 10-4 M.

a)

0.40

b)

3.60

c)

-3.60

d)

10.40

e)

13.60

55.

What is the pH of a 0.400 M HNO3 solution?

a)

0.40

b)

2.05

c)

0.60

d)

4.12

e)

1.67

56.

In the equation

HF + H2O <----> H3O+ + F-

a)

H2O is a base, and HF is its conjugate acid

b)

H2O is an acid, and HF is its conjugate base

c)

HF is an acid, and F- is its conjugate base

d)

HF is a base, and H3O+ is its conjugate acid

e)

HF is a base, and F- is its conjugate acid

57.

Which of the following does not represent a conjugate acid-base pair?

a)

H2O/OH-

b)

H3O+/OH

c)

HCl/Cl-

d)

HNO3/NO3-

e)

NH4+/NH3

58.

According to the Bronsted-Lowry definition, a base

a)

is an electron-pair donor

b)

is an electron-pair acceptor

c)

is a proton donor

d)

is a proton acceptor

59.

What characterizes a strong acid or base?

a)

polar covalent bonding

b)

ionic bonding

c)

presence of a OH- and H+

d)

complete ionization in water

60.

What is the process of adding a known amount of solution of known concentration to determine the concentration of another solution called?

a)

Hydrolysis

b)

Buffer capacity

c)

Neutralization

d)

Titration

61.

Acids have the following properties:

a)

react with metals; feel slippery

b)

are electrolytes; taste sour

c)

taste bitter; feel slippery

d)

taste sour; produce hydroxide ions in solution

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