Given following reduction potentials in solution. Which is weakest oxidising agent in the list. List of numbers on right is for Eo/V.
Al3+(aq)+3e- = Al(s) -1.66
Sn4+(aq)+2e- = Sn2+(aq) +0.14
Is(s)+2e-=21-(aq) +0.53
Why is a certain substance weakest? Is it -1.66 because this is negative compared to the other positive values.
As a reduction (as written). the three potentials represent oxidizing ability. The weakest is Al^+3 because of the -1.66
v
Written as oxidation, Al is the strongest reducing agent because it is +1.66 v.
To determine which substance is the weakest oxidizing agent in the given list, you need to compare the reduction potentials (Eo values).
In electrochemistry, the reduction potential gives an indication of how easily a species can gain electrons and be reduced. The higher the reduction potential, the stronger the oxidizing agent it is, because it is more likely to accept electrons from another substance and cause oxidation.
In your list, the reduction potentials are as follows:
Al3+(aq) + 3e- = Al(s) Eo = -1.66 V
Sn4+(aq) + 2e- = Sn2+(aq) Eo = +0.14 V
I2(s) + 2e- = 2I-(aq) Eo = +0.53 V
Based on these values, the substance with the weakest oxidizing power is Al3+. This is because it has the lowest reduction potential of -1.66 V. The negative value indicates that Al3+ is more likely to lose electrons and be reduced rather than gain electrons and accept reduction. Therefore, it is the weakest oxidizing agent among the substances listed.
In summary, the weakest oxidizing agent is determined by comparing the reduction potentials, and in this case, Al3+ has the lowest reduction potential, making it the weakest oxidizing agent.