For each unbalanced equation below, first decide if it is a Redox equation (some are not). Identify the oxidizing agent and the reducing agent in the Redox equations. The oxidizing agent contains the element that is reduced - gets more negative. The reducing agent contains the element that is oxidized - gets more positive. Hint: oxidizing and reducing agents will always be reactants - NOT products. Under some conditions, the same substance may contain both the element that gains electrons and the element that looses electrons - making it both the oxidizing agent and the reducting agent.

1. SiH2 + O2 → SiO2 + H2O a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   2. H2O2 → H2O + O2 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   3. Fe2O3 + CO → Fe + CO2 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   4. H2SO4 + HI → H2S + I + H2O a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________

5. Ca3(PO4)2 + SiO2 → P4O10 + CaSiO3 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   6. HNO3 + H3PO3 → NO + H3PO4 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   7. MnO4−1 + I−1 → I2 + Mn+2 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________   8. H2O2 + NO2−1 → H2O + NO4−1 a. Is this a Redox equation?   _________ b. The oxidizing agent is __________________ c. The reducing agent is __________________