Questions 2311a. What do the formulas, arrow, and plus signs in a chemical equation tell you?

Questions 2311b. Compare and Contrasting How are reactants and products treated the same in a chemical reaction? How are they treated differently?

Questions 2312a. Explaining How does the idea of atoms explain the principle of conservation of matter?

Questions 2312b. Applying Concepts If the total mass of the products of a reaction is 250g, what was the total mass of the reactants?

Questions 2313a. Reviewing What are three types of chemical reactions?

Questions 2313b. Inferring What is the smallest possible number of products in a decomposition reaction?

Questions 2313c. Classifying Classify the following reaction:P4O10 + 6H2O 4H3PO4

Questions 231Practice__Fe2O3 + __C __Fe + __CO2

__SO2 + __O2 __SO3

Questions 229Balancing Chemical Equations1. Balance the equation for the reaction of sodium metal (Na) with oxygen gas (O2), forming sodium oxide (Na2O).

Questions 229Balancing Chemical Equations2. Balance the equation for the reaction of tin (Sn) with chlorine gas (Cl2), forming tin chloride (SnCl2).

Questions 239Controlling Chemical Equations1a. What is activation energy?

Questions 239Controlling Chemical Equations1B. Describing What role does activation energy play in chemical reactions?

1c. Making Generalizations Look at the diagram in Figure 13, and make a generalization about activation energy in exothermic and endothermic reactions.

Questions 239Controlling Chemical Equations2a. Identifying What are four ways that chemists can control the rates of chemical reactions?

Questions 239Controlling Chemical Equations2b. Applying Concepts Which would react more quickly in a chemical reaction: a single sugar cube or an equal mass of granulated sugar crystals? Explain.

Figure P. 236Energy Changes in Chemical EquationsBoth exothermic and endothermic reactions need energy to get started.Draw and compare the graphs.Figure P. 239Enzyme ActionAfter a reaction, an enzyme molecule is unchanged.