Vocabulary & objectives for building the matter we can see
Percent composition eq
Law of conservation of mass, matter, charge
& energy
Hydrated crystal’s formula
Exothermic
Table J
Mole
Avogadro’s number
Mole calculation eq
Coefficients
Decomposition reaction
Double replacement reaction
Combustion reaction
Anhydrous salt
Endothermic
Empirical formula
Gram formula mass= Molar mass= Formula mass=
Single replacement reaction
Synthesis reaction
Objectives:
1. What does the arrow in a chemical equation mean?
2. Contrast the difference between a plus sign between reactants and a plus sign between products: for
example: CH4 + O2
CO2 + H2O + + 890.4kj
3. How is table J used for single replacement reactions? For example in these unbalanced rxs:
Al
+ CuCl2
AlCl3 + Cu
Vs.
Cu + AlCl3
CuCl2 + Al
4. Compare and contrast synthesis & decomposition reactions. For example
N 2 + 3 H2
2 NH3
vs
NH3
N2 + 3 H2
5. Why do double replacement reactions progress to completion? (Hint which states of matter removed the
products from the reaction?)
6. What types of compounds undergo double replacement?
7. What are the elements in the hydrocarbons of combustion reactions?
8. What is the gas reactant of all combustion reactions? What are the products?
9. If a reaction is endothermic would the energy be a reactant or product?
10. How does adding coefficients allow a reaction to obey conversation laws?
11. What are empirical formulas and how are they useful?
10. Explain the difference between water in a hydrate and water in an aqueous solution.
11. Describe the structure of a hydrated salt?
12. How can the moles of a balanced reaction be useful to a scientist in a lab setting?
13. If the moles are reactants are double what will happen to the moles of product produced?
14 If 2moles of O2 how many moles of CO2 would be produced? CH4 + O2
CO2 + H2O + 890.4kj