Four standard reduction potentials are given below. E red = 0.762 V E red = 2.86

Question

Four standard reduction potentials are given below.

Ered = 0.762 V

Ered = 2.868 V

Ered = 1.662 V

Ered = 0.403 V

(a) Rank the following in order from weakest to strongest oxidizing agent: Zn2+(aq), Ca2+(aq), Al3+(aq), Cd2+(aq). (Use the appropriate <, =, or > symbol to separate substances in the list. Include states-of-matter under the given conditions in your answer.)

(b) Rank the following in order from weakest to strongest reducing agent: Zn(s), Ca(s), Al(s), Cd(s). (Use the appropriate <, =, or > symbol to separate substances in the list. Include states-of-matter under the given conditions in your answer.)

THEN

The oxidation-reduction reaction given below has a standard cell potential. Determine if it is spontaneous or non spontaneous.

Ecell = 1.59 V.

Be2+(aq) + Ni(s) Ni2+(aq) + Be(s)

Zn2+(aq) + 2 e Zn(s)    

Ered = 0.762 V

Ca2+(aq) + 2 e Ca(s)    

Ered = 2.868 V

Al3+(aq) + 3 e Al(s)    

Ered = 1.662 V

Cd2+(aq) + 2 e Cd(s)    

Ered = 0.403 V

Explanation / Answer

oxidizing agent = how well they will perform whlie oxidizing other material, the higher potential to reduce, the stronger oxidizing agent it is

then, from the list:

Cd2+ > Zn2+ > Al3+ > Ca2+

b)

weakest to strong oxidizing agent... this implies which is the hardest to oxidize itself,

Cd2+ < Zn2+ < Al3+ < Ca2+

c)

If the E°cel lvlaue is NEGATIVE, this is not liekly to occur in the forward direction, therefore, it is non spontaneous

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