Download Final Exam Study Guide Page 1 Quiz

Final Exam Study Guide Page 2 Quiz- Key
Sections: The Mole
Stoichiometry
1. Convert 25g of HCl to moles of HCl.
a. .69 moles
b. 887.5 moles
c. 1.5 x 1025 moles
d. none of the above
2. How many grams are in 6.2 moles of NH4?
a. .34 g
b. 111.8 g
c. 6.2 g
d. 11.6 g
3. One mole of CaCO3 is equal to how many molecules of CaCO3?
a. 765 molecules
b. 249 molecules
c. 7.6 x 1024 molecules
d. 6.02 x 1023 molecules
4. How many grams of sodium are required to react with magnesium oxide to
produce 12.3g of magnesium according to the following chemical reaction:
2Na + MgO → Na2O + Mg
a. 28.6 g
b. 33.2 g
c. 23.3 g
d. 13.6 g
5. How many atoms are in 50.2g of Calcium?
a. 1.25 atoms
b. 3.02 x 1025 atoms
c. 7.54 x 1023 atoms
d. 1.21 x 1027 atoms
6. The limiting reactant in a chemical equation:
a. Is completely used up in the reaction
b. Will have some amount unchanged, or leftover, after the reaction
c. Cannot be calculated without performing the reaction
d. Has no effect in the amount of product formed
7. What is the molar mass of H2O?
a. 18 g/mol
b. 36 g/mol
c. 6.02 X 1023 g/mol
d. There is not enough information given
8. Avogadro’s number represents
a. The number of atoms in a mole of an element
b. The number of molecules in a mole of a compound
c. A and B
d. None of the above
Use the following equation to answer numbers 9, 10, and 11:
Fe + 2H2SO4 → Fe(SO4)2 +2 H2
9. If 2.31g iron reacted with 8.83g sulfuric acid, what is the limiting reactant?
a. Fe
b. H2SO4
c. Fe(SO4)2
d. H2
10. Given the amounts above, how much excess reagent remains?
a. 0.0828 moles
b. 0.0042 moles
c. 0.0163 moles
d. 0.0072 moles
11. Given the amounts above, how much iron sulfate can be produced?
a. 8.62 g
b. 10.3 g
c. 12.9 g
d. 9.17 g