Consider the following half-reactions Cu(2+) + 2 e -> Cu E0 = 0.34 V Fe(2+) + 2

Question

Consider the following half-reactions
Cu(2+) + 2 e -> Cu E0 = 0.34 V
Fe(2+) + 2 e -> Fe E0 = -0.44 V
Al(3+) + 3 e -> Al E0 = -1.66 V

In line with the correct characteristics of the best oxidizing/reducing agent, the species that is the best reducing agent is ________________, because when it ____________________(a 5-letter conjugated verb with letter "v" inside) electrons from (to) the other species, and it has the highest ________________(a 9-letter word with a "a" inside) potential:

______________ V. It is followed, in decreasing reducing agent abilities, by

______________ and ______

Explanation / Answer

the given half reactions are

Cu(2+) + 2 e -> Cu E0 = 0.34 V

Fe(2+) + 2 e -> Fe E0 = -0.44 V

Al(3+) + 3 e -> Al E0 = -1.66 V

we know that

reducing agent is the one which undergoes oxidation

so

write the oxidation potentials of the given half reaction

Cu -----> Cu+2 + 2e-   E= -0.34 V

Fe -----> Fe+2 + 2e-     E = 0.44 V

Al -----> Al+3 + 3e-     E = 1.66 V

we know that

the best reducing agent is the one which oxidizes easily

we also know that

higher the oxidation potential easier to undergo oxidation

so

higher the oxidation potential , better the reducing agent

so from the given data

we get

Al is the best reducing agent

the order is

Al > Fe > Cu

so

the answer is

In line with the correct characteristics of the best oxidizing/reducing agent, the species that is the best

reducing agent is Al , because when it gives electrons to the other species, it has the highest oxidation

potential: 1.66 V. It is followed, in decreasing reducing agent abilities, by Fe and Cu

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.