Question

Instructions

Consider the following information when answering Questions 8-10.
Predictions Based Reduction Potentials
Consider the standard reduction potentials.
A13+ (aq) + 3 e-Al (s)
cost log) từ Co2 lag)
-
Cut (aq)+e-Cu (s)
Mn2+ (aq) +2e →Mn (s)
BACKGROUND
Ered=-1.66V
Ered=+1.84 V
Ered=+0.52 V
Ered=-1.18 V
Reduction potential is the tendency for a species to be reduced (gain electrons) in
a reduction half-reaction. Standard reduction potential (Ered) is the voltage
associated with a reduction reaction at an electrode when all solutes are 1 M and
all gases are at 1 atm at 25°C.
The more positive the value of Ered the greater the tendency for reduction under
standard conditions.
.
Large +Ered values (easily reduced, good oxidizing agents)
• Large-Ered values (easily oxidized, good reducing agents)
Standard cell potential (E cell) can be calculated using the standard reduction
9
0.7 points
Using the list of half-reactions and their standard reduction potentials,
answer the following questions.
Part A: Which is the strongest reducing agent?
choose your answer...
Part B: Which is the stro
Part C: Which of the fol
Part D: Which of the fol
choose your answer.....
Cu (s)
Cu* (aq)
Mn³ (aq)
Al (aq)
Al(s)
Co (aq)
Mn (s)
J?

Answer 1

The strongest reducing agent is Al with an Ered of -1.66V, and the strongest oxidizing agent is Co2+ with an Ered of +1.84V. The standard reduction potential values are indicative of the tendency for a species to be reduced or oxidized, influencing their behavior as either reducing or oxidizing agents.

Step-by-step explanation:

When determining the strongest reducing agent and strongest oxidizing agent from a set of half-reactions, we look at the standard reduction potentials (Ered). The species with the lowest (most negative) Ered value acts as the strongest reducing agent because it has a greater tendency to lose electrons. In contrast, the species with the highest (most positive) Ered value acts as the strongest oxidizing agent because it has a greater tendency to gain electrons.

Based on the given data:

• A13+ (aq) + 3 e- → Al (s), Ered = -1.66V
• Co2+ (aq) + 2 e- → Co (s), Ered = +1.84 V
• Cu2+ (aq) + e- → Cu (s), Ered = +0.52 V
• Mn2+ (aq) + 2 e- → Mn (s), Ered = -1.18 V

Part A: Al is the strongest reducing agent (most negative Ered).

Part B: Co2+ is the strongest oxidizing agent (most positive Ered).

Applying this concept to predict the spontaneity of redox reactions, a reaction is spontaneous if the cell potential (Ecell) is positive, which occurs when Ered cathode > Ered anode. Hence, a species higher in the table (with higher Ered) is a stronger oxidant than one lower in the table.