This document discusses: 1) Transforming worded chemical equations into balanced chemical equations. Examples include iron reacting with bromine to form iron bromide and hydrogen chloride splitting into hydrogen and chlorine. 2) Classifying chemical equations as synthesis, analysis, single replacement, or double replacement reactions. Examples classified include ammonia forming from nitrogen and hydrogen (analysis) and calcium oxide reacting with carbon dioxide to form calcium carbonate (synthesis). 3) Calculating the molar mass of various compounds from their chemical formulas. Examples given are the molar mass of copper(II) sulfate, tin(III) chloride, magnesium oxide, sulfuric acid, and aluminum sulfide.

1. Activity on Molar Mass, Equation, and Reaction
I. Transform the worded equations completely into a chemical equation.
1. Iron reacted with bromine to form the resulting compound.
Fe + Br2 FeBr3
2. Cupric oxide decomposed into its constituent elements.
CuO Cu+O2
3. Sodium reacts with oxygen forming sodium oxide.
Na+ O2 Na2O
4. Hydrogen chloride splits into hydrogen and chlorine.
HCl H+Cl
5. Nitrogen and hydrogen formed its corresponding product.II.
H2 + N2 NH3
3H2+ N2 2NH3 Ammonia
Complete and classify the following equations as to type of chemical reaction such
as
A(Synthesis) B(Analysis) C(Single Replacement) D(Double Replacement). Use
letters only.
1. NH3 N2 + H2 B
2.CaO + CO2
CaO + CO2→CaCO3 A
3. HF H2 + F2 B
4. H20 + CO2
H20 + CO2 H2CO3 A
5. C2H5OH + O2III 2CO2 +3H2O C
Determine the molar mass of the following.
1. CuSO4 159.60 g/mol
2. SnCl3 225.069 g/mol

2. 3. MgO 40.30 g/mol
4. H2SO3 82.07 g/mol
5. Al2S3 150.16 g/mol