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Assessment - Mole, Mass, Volume & # of Atoms/Molecules/Particles

Total questions: 40

Worksheet time: 6hrs 37mins

Name
Class
Date
1.

What is the mass, in grams, of 4.725 mole of aluminum oxide Al2O3?{Al = 27, O = 16}

a)

964 g

b)

482 g

c)

1928 g

2.

How many moles of iron (III) oxide are contained in 276 g of pure Fe2O3? {Fe = 56, O = 16}

a)

0.57 moles

b)

1.71 moles

c)

3.42 moles

3.

It states that “equal volumes of gases at the same temperature and pressure contain equal numbers of particles”.

a)

Avogadro's hypothesis

b)

Newton's hypothesis

c)

Bohr's hypothesis

4.

At STP, 1 mol, or representative particles, of any gas occupies a volume of......................

a)

24.4 L

b)

44.2 L

c)

22.4 L.

5.

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

a)

13 L

b)

26 L

c)

6.5 L

6.

A student wants to convert 7.3 x 1022 molecules of water to moles of water. Which of the following should be the next step in the calculation?

a)

6.022 x 1023 molecules / 1 mol

b)

18.01 g / 1 mol

c)

1 mol / 6.022 x 1023 molecules

d)

1 mol / 18.01 g

7.

How many atoms are in 0.34 moles of strontium?

a)

2.0 x 1023 atoms of Sr

b)

5.7 x 1023 atoms of Sr

c)

1.2 x 1023 atoms of Sr

d)

5.0 x 1022 atoms of Sr

8.

How many molecules of dinitrogen pentoxide are in 1.44 moles of dinitrogen pentoxide (N2O5)?

a)

3.56 x 10-24 molecules N2O5

b)

2.39 x 10-24 molecules N2O5

c)

8.67 x 1023 molecules N2O5

d)

4.23 x 1023 molecules N2O5

9.

Convert 3.55 grams potassium to atoms. (Molar Mass K = 39.10 g/mol)

a)

2.67 x 1022 atoms K

b)

5.47 x 1022 atoms K

c)

8.36 x 1025 atoms K

d)

1.51 x 10-25 atoms K

10.

Convert 6.7 grams of aluminum sulfate (Al2(SO4)3) to moles. (Molar Mass Al2(SO4)3 = 342.15 g/mol)

a)

0.020 mol Al2(SO4)3

b)

2.3 x 103 mol Al2(SO4)3

c)

0.039 mol Al2(SO4)3

d)

4.0 x 103 mol Al2(SO4)3

11.

The molar mass of water is 18.02 g/mol. How many grams is 3 moles of water?

a)

6.01 g

b)

.166 g

c)

54.06 g

d)

76.01 g

12.

Calulate the volume of .70 moles of hydrogen gas (H2).

a)

7.84 L

b)

32.00 L

c)

15.68 L

d)

.03 L

13.

Calculate the number of moles in 12.00 L of gas.

a)

3.73 mol

b)

1.87 mol

c)

268.80 mol

d)

.54 mol

14.

How many moles are in 7.90 L of a gas?

a)

.35 mol

b)

.705 mol

c)

88.48 mol

d)

176.96 mol

15.

How many moles are in 225g of CO?

a)

9.1 mole

b)

8.04

c)

4.82x1024 mole

d)

7.50 mole

16.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
17.

How many moles are there in 440g of carbon dioxide (CO2)?

a)

11

b)

10

c)

16

d)

0.25

18.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
19.
There are ______ number of molecules (atoms) of NaCl in one mole of NaCl?
a)
6.02 x 1023
b)
1 mole
c)
2
d)
Mr. Miller
20.
The best definition for a mole provided below is
a)
The unit for the mass of something
b)
The unit for the amount of a substance
c)
The unit for the volume of something
d)
The unit for the area of a substance
21.
Which list of number of atoms in Mg(NO2)2 is right?
a)
Mg : 1--NO :  2
b)
Mg : 1-- N :  6--O:  2
c)
Mg :  1-- N:   1--  O: 2
d)
Mg :  1-- N: 2--  O: 4
22.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

23.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
24.

What is true about 1 mole of gold and 1 mole of water?

a)

They have the same mass.

b)

They have the same number of particles.

c)

They have the same volume.

d)

Nothing is the same.

25.

What is the value and units of Avogadro's number?

a)

it depends on the substance.

b)

6.02 x 1023 particles = 1 mole

c)

6.02 x 1023 grams = 1 mole

d)

18.02 particles = 1 mole

26.

Which is the correct conversion factor to go FROM 5 moles TO atoms of carbon?

a)

12.01 g / 1 mol

b)

6.02 x 1023 atoms / 1 mol

c)

1 mol/ 12.01 g

d)

1 mol/ 6.02 x 1023 atoms

27.

Mylanta, a common antacid, contains magnesium hydroxide, Mg(OH)2. How many moles of magnesium hydroxide are in 75.0 g of magnesium hydroxide?

a)

0.551 moles

b)

0.778 moles

c)

1.29 moles

d)

1.82 moles

28.

Which has more molecules?

a)

1 mole H

b)

1 mole Al(OH)3

c)

1 mole LiBr

d)

There are all the same

29.
Calculate the number of oxygen atoms present in 14kg of Ba(NO3)2
a)
53.578 atoms
b)
3.22x1025 atoms
c)
3.22x1022 atoms
d)
6.44x1022 atoms
30.
Calculate the mass of iron in a sample of iron ore containing 2.61x1023 iron atoms.
a)
0.433g
b)
24.2g
c)
44g
d)
6.02g
31.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
32.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

33.
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 
34.
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

35.

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

a)

40 g

b)

80 g

c)

16 g

d)

32 g

36.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
37.
Which of the following dimensional analysis setups will correctly convert 2.50 moles of sodium to grams of sodium?
a)
A
b)
B
c)
C
d)
D
38.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
39.

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

40.

Match the following units to their correct category.

a)

Grams

1.

Mass

b)

Liters at STP

2.

Volume

c)

Units, Atomes, Molecules

3.

Particles

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