Untitled - Kelly Walsh High School

Mass, Moles, and Equations 45
7. The amount of product calculated to form in a reaction is the __________.
8. The simplest whole-number ratio of the elements present in a compound is
the __________.
9. Balance the following chemical equations:
a. ___ N2(g) ___ O2(g) l ___ N2O5(s) b. ___ CoCl2(s) ___ ClF3(g) l ___ CoF3(s) ___ Cl2(g) c. ___ La(OH) 3(s) ___ H2C2O4(aq) l ___ La2(C2O4) 3(s) ___ H2O(l) d. ___ C4H10(g) ___ O2(g) l ___ CO2(g) ___ H2O(g) e. Ammonia gas, NH3, reacts with fluorine gas, F2, to form nitrogen gas, N2, and gaseous hydrogen fluoride, HF.
10. Balance the following chemical equations:
a. ___ Br2(l) ___ O2(g) l ___ Br2O3(s) b. ___ PF3(l) ___ H2O(l) l ___ H3PO3(aq) ___ HF(aq)
c. ___ Zn(OH) 2(s) ___ H3VO4(aq) l ___ Zn3(VO4) 2(s) ___ H2O(l) d. ___ C6H14(l) ___ O2(g) l ___ CO2(g) ___ H2O(l) e. Methane gas, CH4, reacts with chlorine gas, Cl2, to produce liquid carbon
tetrachloride, CCl4, and gaseous hydrogen chloride, HCl.
11. Convert each of the following to empirical formulas.
a. hydrogen peroxide, H2O2 b. glucose, C6H12O6 c. Ethane, C2H6 d. nitric acid, HNO 3
e. ammonium peroxydisulfate, (NH 4) 2S 2O 8
12. Determine the molar mass of each of the following to two decimal places.
a. H 2O b. CO 2 c. HNO 3 d. Na 2SO 4 e. (NH 4) 3PO 4
13. How many moles of material are present in 100.00 g of each of the following?
a. H 2O b. CO 2 c. HNO 3 d. Na 2SO 4 e. (NH 4) 3PO 4
14. How many grams are present in 2.50 mol of each of the following?
a. H 2O b. CO 2 c. HNO 3 d. Na 2SO 4 e. (NH 4) 3PO 4
15. You are given 3.00 mol of second reactant in each of the reactions in question
number 9. How many moles of the first product will form in each
case?
16. You are given 3.00 mol of each reactant in each of the reactions in question
10. Which of the reactants is the limiting reactant?
17. You are given 3.00 mol of each reactant in each of the reactions in question
10. What is the percent yield if 10.0 g of the first product forms?
18. The analysis of a gas sample found 21.4 g of sulfur and 50.8 g of fluorine.
Determine the empirical formula of this compound.
19. Analysis of a dark brown solid showed 69.6% manganese, Mn, and 30.4%
oxygen, O. Determine the empirical formula of the compound. (Hint:
assume you have 100 g of sample. This means that 69.6% Mn is 69.6 g of
Mn, and that 30.4% O is 30.4 g O.)
20. A gaseous sample with a molar mass of approximately 254 g/mol was found
to consist of 25.2% sulfur, S, and 74.8% fluorine, F. What is the molecular
formula of this sample?