Question
Calculate the cell potentials for this reaction and state whether it is feasible or not. 2Al(s) + 2Sn^4+(aq)=2Al^3+ (aq) + 3Sn^2+(aq).
Which is the oxidizing agent and which is the reducing agent
Which is the oxidizing agent and which is the reducing agent
Answers
GPT 3.5
The half-reactions for this reaction are:
1. Al(s) -> Al^3+(aq) + 3e- (oxidation)
2. Sn^4+(aq) + 2e- -> Sn^2+(aq) (reduction)
The standard reduction potentials for these half-reactions are:
1. Al^3+(aq) + 3e- -> Al(s) E° = -1.66 V
2. Sn^4+(aq) + 2e- -> Sn^2+(aq) E° = 0.15 V
The balanced overall reaction can be written as:
2Al(s) + 2Sn^4+(aq) -> 2Al^3+(aq) + 3Sn^2+(aq)
The overall cell potential (E°cell) can be calculated as:
E°cell = E°cathode - E°anode
E°cell = 0.15 V - (-1.66 V) = 1.81 V
Since the calculated cell potential is positive (1.81 V), the reaction is feasible.
In this reaction, Al is the reducing agent and Sn^4+ is the oxidizing agent.
1. Al(s) -> Al^3+(aq) + 3e- (oxidation)
2. Sn^4+(aq) + 2e- -> Sn^2+(aq) (reduction)
The standard reduction potentials for these half-reactions are:
1. Al^3+(aq) + 3e- -> Al(s) E° = -1.66 V
2. Sn^4+(aq) + 2e- -> Sn^2+(aq) E° = 0.15 V
The balanced overall reaction can be written as:
2Al(s) + 2Sn^4+(aq) -> 2Al^3+(aq) + 3Sn^2+(aq)
The overall cell potential (E°cell) can be calculated as:
E°cell = E°cathode - E°anode
E°cell = 0.15 V - (-1.66 V) = 1.81 V
Since the calculated cell potential is positive (1.81 V), the reaction is feasible.
In this reaction, Al is the reducing agent and Sn^4+ is the oxidizing agent.