Answer:
In Table 6.1, the initial solutions of each metal are provided: Cu(NO3)2, Fe(NO3)3, and Zn(NO3)2. The table is asking for the results of the oxidation-reduction reactions that occur when these metals are reacted with each other.
In Table 6.2, the metals (Cu, Fe, Zn) are listed, and the table is asking whether each metal was oxidized or not, and what oxidizing agent(s) were involved in the reaction.
1. Zn is the most reactive metal because it readily undergoes oxidation when in contact with other metals. This is known as the activity series of metals.
2. The order of increasing reactivity is Cu, Fe, Zn.
3. The chemical equations for each single replacement reaction are:
Cu + Zn(NO3)2 → Cu(NO3)2 + Zn
Fe + Cu(NO3)2 → Fe(NO3)2 + Cu
Zn + Fe(NO3)3 → Zn(NO3)2 + Fe
4. Fe was reduced, and Cu and Zn acted as reducing agents.
Step-by-step explanation: