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Mid MP 3 Chemistry Exam

Total questions: 90

Worksheet time: 2hrs 39mins

Name
Class
Date
1.

What is the first step in converting grams to moles?

a)

Divide the grams by the molar mass

b)

Add the grams to the molar mass

c)

Find the molar mass of the substance

d)

Multiply the grams by the molar mass

2.

What does the molar mass represent?

a)

The density of a substance

b)

The volume of one mole of a substance

c)

The mass of one mole of a substance

d)

The number of atoms in a molecule

3.

Which unit is used for molar mass?

a)

Liters per mole (L/mol)

b)

Moles per gram (mol/g)

c)

Kilograms per mole (kg/mol)

d)

Grams per mole (g/mol)

4.

What is the molar mass of nitrogen (N)?

a)

68.17 g/mol

b)

32.07 g/mol

c)

1.01 g/mol

d)

14.01 g/mol

5.

What is the molar mass of hydrogen (H)?

a)

1.01 g/mol

b)

14.01 g/mol

c)

32.07 g/mol

d)

68.17 g/mol

6.

What is the molar mass of sulfur (S)?

a)

32.07 g/mol

b)

1.01 g/mol

c)

68.17 g/mol

d)

14.01 g/mol

7.

What is the molar mass of ammonium sulfide ((NH4)2S)?

a)

68.17 g/mol

b)

32.07 g/mol

c)

14.01 g/mol

d)

1.01 g/mol

8.

How many moles are in 2 grams of ammonium sulfide (NH4)2S?

a)

2.93 mol

b)

0.00293 mol

c)

0.293 mol

d)

0.0293 mol

9.

What is a mole ratio?

a)

The ratio between the masses of two substances in a chemical reaction

b)

The ratio between the amounts in moles of any two substances in a chemical reaction

c)

The ratio between the densities of two substances in a chemical reaction

d)

The ratio between the volumes of two substances in a chemical reaction

10.

What is the first step in finding the mole ratio?

a)

Balance the chemical equation

b)

Convert the units

c)

Identify the substances

d)

Write the ratio

11.

Which of the following is essential for determining the mole ratio?

a)

The physical states of the substances

b)

The molecular weights of the substances

c)

The coefficients of the balanced chemical equation

d)

The temperature of the reaction

12.

How is the mole ratio written?

a)

As a ratio of masses

b)

As a percentage

c)

As a fraction or in the format 'X:Y'

d)

As a decimal

13.

In the reaction 2H2(g)+O2(g) --> 2H2O(g), what is the mole ratio of H2 to O2?

a)

2:1

b)

1:2

c)

1:1

d)

2:2

14.

In the reaction 2H2(g)+O2(g) --> 2H2O(g), what is the mole ratio of O2 to H2O?

a)

2:2

b)

1:1

c)

2:1

d)

1:2

15.

What does the mole ratio act as in stoichiometry?

a)

A conversion factor

b)

A chemical catalyst

c)

A balancing tool

d)

A measurement device

16.

What is the purpose of using a mole ratio in calculations?

a)

To relate the quantities of reactants and products

b)

To determine the physical state of substances

c)

To measure the temperature of the reaction

d)

To calculate the density of substances

17.

What is the purpose of balancing a chemical equation before finding the mole ratio?

a)

To measure the temperature of the reaction

b)

To calculate the molecular weights

c)

To determine the physical states of substances

d)

To ensure the coefficients are correct

18.

What is the mole ratio used for in stoichiometry problems?

a)

To calculate the amount of one substance needed or produced from another

b)

To measure the density of substances

c)

To determine the physical states of substances

d)

To balance the chemical equation

19.

Match the following substances to their correct mole ratios using the balanced chemical equation below:

1 Al2(SO4)3 +  6 NaOH → 2 Al(OH)3 + 3 Na2SO4

a)

Al2(SO4)3 & NaOH

1.

1:6

b)

NaOH & Al(OH)3

2.

6:2

c)

Al(OH)3 & Na2SO4

3.

2:3

d)

Na2SO4 & Al2(SO4)3

4.

3:1

20.

3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe

Identify the mole ratios for the following pairs:

​ ​ ​ (a)   Mg : ​ (b)   Fe

​ (c)   Fe2O3 : ​ (d)   Fe

​ 1 Fe2O3 : ​ (e)   MgO

Choose from the below words
3
2
1
21.
In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?
a)
10:6 
b)
3:4
c)
4:3
d)
2:3
22.
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
23.
What is the mole ratio in the following reaction:
2CO  +  O2  → 2CO2
a)
2:1:2
b)
1:1:1
c)
1:2:1
d)
Have no clue what a mole ratios is!!
24.

Mole Ratios used for conversions are derived from:

a)

the molar mass of the reactants in the balanced chemical equation

b)

the coefficients of the balanced chemical equation

c)

the subscripts of the products in the balanced chemical equation

d)

the group number of each element in the balanced chemical equation

25.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of NO produced when 1 mole of O2 is completely consumed?
a)
1
b)
1.2
c)
0.8
d)
4
26.
H2+Cl2-->2HCl
How many moles of Cl2 is needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
27.

What is the mole ratio of Mg to MgCl2?

Mg(s) + HCl(aq) → MgCl2(aq) + H2(g)

a)

2 mol Mg/ 1 mol MgCl2

b)

1 mol Mg/ 2 mol MgCl2

c)

1 mol Mg/ 1 mol MgCl2

d)

2 mol Mg/ 2 mol MgCl2

28.

Using the reaction below,

4Al + 3O2 → 2Al2O3

How many moles of aluminum oxide are produced from 6 moles of oxygen?

a)

8 mol

b)

6 mol

c)

4 mol

d)

2 mol

29.

Using the balanced equation:

2 HBr + Ca(OH)2 --> H2O + CaBr2


What is the mole ration between H2O and HBr?

a)

1 mol H2O / 2 mol HBr

b)

2 mol H2O / 1 mol HBr

c)

1 mol H2O / 1 mol HBr

30.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
d)
our minds
31.

What is the mass on this triple beam balance?

a)
200g
b)
44g
c)
244g
d)
4g
32.

What is the mass on this triple beam balance?

a)
143g
b)
40g
c)
43g
d)
3g
33.

What is the mass on this triple beam balance?

a)
142g
b)
42g
c)
102g
d)
444g
34.

What is the mass on this triple beam balance?

a)

272.1g

b)
702g
c)
202g
35.

What is the mass of this object?

a)

615.3 grams

b)

516 grams

c)

165.3 grams

d)

165.3 inches

36.

What is the mass of this object?

a)

421.5 grams

b)

241.5 grams

c)

1.524 grams

d)

421.5 inches

37.

What is the mass of this object?

a)

58 grams

b)

85 grams

c)

185 grams

d)

80.5 grams

38.

What is the mass of this object?

a)

328 grams

b)

300.2.8 grams

c)

333 grams

d)

302.8 grams

39.

What is the mass of this object?

a)

320.5 grams

b)

321 grams

c)

231.5 grams

d)

230.5 grams

40.
How would you read this triple beam balance?
a)
34 g
b)
40.3 g
c)
143 g
d)
43 g
41.

What is the mass of this object?

a)

111.5 grams

b)

1.5 grams

c)

2 grams

d)

1 gram

42.

The mass on the triple beam balance is (a)   .

Choose from the below words
345.5
304.5
700.5
43.

What is the value on the balance?

a)

270.0 g

b)

202.1 g

c)

272.1 g

d)

200.0 g

44.

Read the mass shown on the triple beam balance below to the nearest tenth of a gram. You must include g in your answer

(a)  

45.

What is the function of the pan on a triple beam balance?

a)

To hold the object being weighed

b)

To adjust the zero mark

c)

To slide the riders

d)

To measure the mass of the object.

46.

Fill in the blank: The _______ is used to adjust the balance to zero before weighing an object.

a)

Pan

b)

Zero Adjustment Knob

c)

Pointer

d)

Rider

47.

Which part of the triple beam balance holds the riders?

a)

Pan

b)

Beams

c)

Pointer

d)

Zero Adjustment Knob

48.

What is the purpose of the riders on a triple beam balance?

a)

To hold the object

b)

To measure the mass

c)

To adjust the zero mark

d)

To balance the beams.

49.

Fill in the blank: The back beam has a 100 g scale with a _______ g rider.

a)

0.1

b)

10

c)

50

d)

100

50.

What should you do first to ensure the balance is calibrated?

a)

Place the object on the pan

b)

Slide all riders to the leftmost positions

c)

Adjust the zero mark

d)

Weigh the object.

51.

Fill in the blank: The middle beam has a 500 g scale with a _______ g rider.

a)

0.1

b)

10

c)

100

d)

500

52.

What is the next step after placing the object on the pan?

a)

Adjust the zero mark

b)

Slide the 100-gram rider

c)

Slide the 10-gram rider

d)

Read the measurement.

53.

Fill in the blank: The front beam has a 10 g scale with a _______ g rider.

a)

0.1

b)

1

c)

10

d)

100

54.

What should you do if the pointer drops below the zero mark while sliding the 100-gram rider?

a)

Move the rider back one notch

b)

Slide the 10-gram rider

c)

Adjust the zero mark

d)

Weigh the object again.

55.

Fill in the blank: The _______ is used to indicate when the balance is level.

a)

Pan

b)

Pointer

c)

Rider

d)

Beam

56.

What is the final step in using a triple beam balance?

a)

Adjust the zero mark

b)

Slide the 0.1-gram rider

c)

Add the values of all three beams

d)

Place the object on the pan.

57.

Fill in the blank: The zero adjustment knob is located _______ the pan.

a)

Above

b)

Below

c)

Beside

d)

On

58.

What is the role of the notch on the beams?

a)

To hold the object

b)

To adjust the zero mark

c)

To stop the riders

d)

To measure the mass.

59.

Fill in the blank: The triple beam balance is used to measure the _______ of an object.

a)

Length

b)

Volume

c)

Mass

d)

Temperature

60.

This is a ​ (a)   . It measures ​ (b)   . It's units are ​ (c)   .

Choose from the below words
triple beam balance
mass
grams (g)
hot plate
volume
liters (L)
61.

What is the formula used to convert moles to grams?

a)

Grams = Moles ÷ Molar Mass

b)

Grams = Moles × Molar Mass

c)

Grams = Moles + Molar Mass

d)

Grams = Moles - Molar Mass

62.

What unit is the molar mass typically expressed in?

a)

grams

b)

moles

c)

grams per mole (g/mol)

d)

moles per gram

63.

Which tool is used to find the atomic mass of an element?

a)

Calculator

b)

Periodic Table

c)

Thermometer

d)

Ruler

64.

If you have 1 mole of a substance, how many grams do you have?

a)

The same as the molar mass

b)

1 gram

c)

0 grams

d)

100 grams

65.

What is the first step in converting moles to grams?

a)

Multiply by the atomic number

b)

Find the number of moles given

c)

Add the number of atoms

d)

Divide by the molar mass

66.

What does the subscript in a chemical formula indicate?

a)

The number of molecules

b)

The number of atoms of that element

c)

The number of moles

d)

The number of grams

67.

What happens to the "moles" unit when you multiply moles by molar mass?

a)

It remains in the answer

b)

It cancels out

c)

It doubles

d)

It becomes grams per mole

68.

What is the molar mass of hydrogen ( HH ) to two decimal places?

a)

1.00 g/mol

b)

1.01 g/mol

c)

2.00 g/mol

d)

16.00 g/mol

69.

What is the molar mass of oxygen ( OO ) as used in the example?

a)

1.01 g/mol

b)

2.02 g/mol

c)

16.00 g/mol

d)

18.02 g/mol

70.

How do you calculate the total molar mass of a compound?

a)

Add the atomic numbers

b)

Add the atomic masses of all atoms in the formula

c)

Multiply the number of moles by the atomic mass

d)

Subtract the atomic masses

71.

What is the molar mass of water ( H2OH_2O ) as calculated in the example?

a)

2.02 g/mol

b)

16.00 g/mol

c)

18.02 g/mol

d)

36.04 g/mol

72.

If you have 2.00 moles of water, how many grams do you have?

a)

18.02 grams

b)

2.00 grams

c)

36.04 grams

d)

16.00 grams

73.

What is the correct sequence of steps to convert moles to grams?

a)

Find moles, multiply by atomic number, add results

b)

Find moles, determine molar mass, multiply, calculate

c)

Find grams, divide by molar mass, subtract

d)

Find moles, add atomic masses, divide

74.

If a compound has a formula AB2AB_2 , how do you find its molar mass?

a)

Add atomic mass of A and B

b)

Add atomic mass of A and twice the atomic mass of B

c)

Multiply atomic mass of A by 2

d)

Subtract atomic mass of B from A

75.

What is the unit for the final answer when converting moles to grams?

a)

Moles

b)

Grams

c)

Moles per gram

d)

Grams per mole

76.

If you are given the number of moles and the molar mass, what operation do you perform to find grams?

a)

Addition

b)

Subtraction

c)

Multiplication

d)

Division

77.

What is the atomic mass of hydrogen ( HH ) used in the example?

a)

1.01

b)

2.02

c)

16.00

d)

18.02

78.

How many hydrogen atoms are in one molecule of water ( H2OH_2O )?

a)

1

b)

2

c)

3

d)

0

79.

How many oxygen atoms are in one molecule of water ( H2OH_2O )?

a)

1

b)

2

c)

3

d)

0

80.

If the molar mass of a compound is 50 g/mol, how many grams are in 3 moles?

a)

150 grams

b)

53 grams

c)

47 grams

d)

15 grams

81.

What is the purpose of multiplying the atomic mass of each element by the number of atoms in the formula?

a)

To find the number of molecules

b)

To find the total mass contributed by that element

c)

To find the number of moles

d)

To find the number of electrons

82.

If you have 0.5 moles of a substance with a molar mass of 20 g/mol, how many grams do you have?

a)

10 grams

b)

20 grams

c)

0.5 grams

d)

40 grams

83.

What is the subscript of oxygen in H2OH_2O ?

a)

2

b)

1

c)

0

d)

3

84.

If a compound’s formula is C6H12O6C_6H_{12}O_6 , how many oxygen atoms are in one molecule?

a)

6

b)

12

c)

1

d)

18

85.

If you have 4 moles of a substance with a molar mass of 10 g/mol, how many grams do you have?

a)

40 grams

b)

14 grams

c)

4 grams

d)

10 grams

86.

What is the atomic mass of oxygen ( OO ) as used in the calculation for water?

a)

1.01

b)

2.02

c)

16.00

d)

18.02

87.

If you have 0.25 moles of a compound with a molar mass of 44 g/mol, how many grams do you have?

a)

11 grams

b)

44 grams

c)

0.25 grams

d)

22 grams

88.

What is the result of 2.00 moles×18.02 g/mol2.00 \text{ moles} \times 18.02 \text{ g/mol} ?

a)

18.02 grams

b)

36.04 grams

c)

2.00 grams

d)

16.00 grams

89.
How many oxygen atoms are in this chemical formula?
a)
6 oxygen atoms
b)
2 oxygen atoms
c)
3 oxygen atoms
d)
4 oxygen atoms
90.

Look at the picture of the chemical formula. Which chemical formula matches what you see in the image?

a)

2H2O2H_2O

b)

H4O2H_4O_2

c)

4H2O4H2O

d)

2HO2HO

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