Hello! I'll help you understand the spontaneity of the redox reactions provided.
In redox reactions, spontaneity is determined by the standard cell potential (E°cell) of the reaction. The greater the E°cell value, the more spontaneous the reaction.
Let's evaluate the provided reactions:
1) Fe (s) + Pb2+ (aq) = Fe2+ (aq) + Pb (s)
2) Fe (s) + Mg2+ (aq) = Fe2+ (aq) + Mg (s)
To determine which reaction is spontaneous, we need to look at the standard reduction potentials for each half-reaction involved in the redox reactions. By comparing the reduction potentials, we can calculate the E°cell for each reaction.
Based on the reduction potentials:
- The reduction potential for Fe2+/Fe is higher than that for Pb2+/Pb.
- The reduction potential for Mg2+/Mg is higher than that for Fe2+/Fe.
This means:
- Reaction 1 is spontaneous because Fe2+ can reduce Pb2+.
- Reaction 2 is also spontaneous because Fe2+ can reduce Mg2+.
Therefore, the correct statement is: Both Eq: 1 and Eq: 2 are spontaneous redox reactions.
