Michele Dell’Aquila
Mole Quiz
1. What is the Mole?
A) The SI unit used to measure the amount of a substance.
B) The SI unit used to measure the charge of a substance.
C) A kind of particle.
D) 1 gram of Carbon.
2. Which is Avogadro’s number?
A) 6.222
B) 6.022 x 1021
C) 6.022 x 1023
D) 6.023
3. What is Avogadro’s number?
A) The number of moles in 1.000 moles.
B) The number of atoms or molecules in 1.000 moles.
C) The weight of 2.000 mole.
D) The volume of the atoms in 1 mole.
4. Is the Mole a Counting Unit?
A) Yes
B) No
5. What is the Molar Mass?
A) The weight on the periodic table of a substance.
B) The mass in grams of 10 moles of a substance.
C) The weight in grams of a substance.
D) The mass in grams of 1 mole of a substance.
6. Molecular Weight is
A) The weight of a molecule measured in Amu.
B) The mass of a molecule measured in grams.
C) The weight of a molecule measured in grams.
D) The length of a molecule measured in centimetres .
7. Formula Weight is
A) The weight of a molecule in Amu.
B) The weight of a simplest ratio of cations to anions of an ionic
compound in Amu.
C) The mass of a simplest ratio of cations to anions of an ionic
compound in grams.
D) The mass of an atom in Amu.
8. The easiest way to recognize a ionic compounds is
A) To check for the presence of a metal.
B) To check for the presence of a molecule.
C) To check for the presence of a non-metal.
D) To check for the presence of water.
9. Can Amu be converted to g/mol ?
A) Yes. Multiplying it for 6.022 x 1023.
B) No.
C) Only dividing by 6.022 x 1023
D) Yes. The numerical value is the same.
10. The Molar Mass of H is:
A) 6.022 g/mol
B) 1.01 g/mol
C) 1.001 g/mol
D) 7.06 g/mol
11. Find the number of sodium ions in 5.12 mole NaNO3.
A) 5.56 x 1022 Na+ ions.
B) 6.45 x 1021 Na+ ions.
C) 3.08 x 1024 Na+ ions.
D) 3.009 x 1024 Na+ ions.
12. Find the mass in grams of 3.012 x 1024 ions Ca+2, 40.08 g/mol
A) 4.45 x 10-4 g Ca+2
B) 200.5 g Ca+2
C) 44 g Ca+2
D) 565 g Ca+2
13. Find the mass in grams of 5.710 x 1023 molecules CH4 , 16.05 g/mol.
A) 432 g CH4
B) 15.22 g CH4
C) 15.2 g CH4
D) 15.6 g CH4
14. Find the mass in grams 4.30 x 1016 atoms He, 4.00 g/mol
A) 445 g He
B) 3.24 x 10-7 g He
C) 2.26 x 10-7 g He
D) 2.86 x 10-7 g He
15. What is the mass of 6.022 x 1023 molecules of ibuprofen (206.31 g/mol)
A) 534 g ibuprofen
B) 234 g ibuprofen
C) 206.3 g ibuprofen
D) 206.31 g ibuprofen
16. How many atoms of Fe are in the formula Fe3C? How many moles of Fe are in
one mole of Fe3C?
A) 3 atoms, 6 moles
B) 6 atoms, 3 moles
C) 1 atom, 1 mole
D) 3 atoms, 3 moles
17. Determine the molecular formula for a compound with the empirical formula
CoC4O4 and a molar mass of 341.94 g/mol.
A) CO2C8O8
B) CO2CO
C) C2OCO
D) CO2C2O8
18. The element bromine is distributed between two isotopes. The first, amounting
to 50.69%, has a mass of 78.918 amu. The second amounting to 49.31%, has a
mass of 80.916 amu. Calculate the average atomic mass of bromine.
A) 80.9 amu
B) 79.90 amu
C) 79.8 amu
D) 44.3 amu
19. A compound of silver has the following analytical composition: 63.50% Ag,
8.25% N, 28.25% O. Calculate the empirical formula.
A) AgNO
B) AgNO2
C) Ag2NO
D) AgNO3
20. Chlorine gas is a diatomic molecule, Cl2. There are 6.00 mol of chlorine atoms in
a sample of chlorine gas. How many moles of chlorine gas molecules is this?
A) 4.00 mol Cl2
B) 2.00 mol Cl2
C) 6.00 mol Cl2
D) 3.00 mol Cl2
Answer key
1.
2.
3.
4.
5.
6.
A
C
B
A
D
A
7. B
8. A
9. D
10. B
11. C
12. B
13. B
14. D
15. C
16. D
17. A
18. B
19. D
20. D