Lesson #2: Using the Redox TablePart I: PracticeFor each of the following reactions, write the half-cell reactions and label them asoxidation or reduction.1. Pb(s) + Cu +2 (aq) ----------- Pb +2 (aq) + Cu(s)2. 2Ag(s) + Pb +2 (aq) ----------------- 2Ag + (aq) + Pb(s)Part II: Redox TableQ: What do we use the Redox table for?A:1. To predict the __________________ Redox reaction to occur.2. To write the _______________ equation for the Redox reaction.3. To predict whether the reaction is spontaneous or non-spontaneous.Q: What’s the difference between oxidation and oxidizing agent?A: Oxidation is the process of losing electrons in a Redox reaction, whereas an oxidizingagent is a chemical species that ____________________ away from another chemicalspecies (i.e., the oxidizing agent causes oxidation of the other species)A reducing agent is a chemical species that _________________ to another chemicalspecies (i.e., the reducing agent causes the reduction of the other species)Rule: The most likely reaction to occur is always between the ______________oxidizing agent and the strongest reducing agent.