19. Given the following pair of half reactions, what is the standard cell potent

19. E0cell = -1.18- (-1.66) = 0.48 V 20. Ecell = E0cell - (0.0591/n)log(Al^3+)^2 / (Zn^2+)^3 = 0.9-(0.0591/6)log(1.5^2/0.1^3) = 0.867 v b. 0.867 v

ID: 964625 • Letter: 1

Question

19. Given the following pair of half reactions, what is the standard cell potential, E°cell, for the spontaneous reaction?

Mn2+ (aq) + 2e- à Mn (s) E°= -1.18V

Al3+ (aq) + 3e- à Al (s) E°= -1.66

a. +0.22 V

b. -0.22 V

c. -0.48 V

d. +2.84 V

e. +0.48 V

20. Calculate the cell potential, Ecell, for the redox reaction below at 25°C if the concentration arc is as follows:

[Zn2+] = 0.100 M and [Al3+]= 1.50 M

3 Zn2= (aq) + 2 AL (s) à 3 Zn (s) + 2 Al3+ (aq) E°= +0.900 V

a. 0.800 V

b. 0.867 v

c. 0.912 V

d. 0.933 V

e. 0.834 V

21. In the voltaic cell shown below, which direction would the indicated species travel?

Anode Cathode

Electrons Cations Anions

a. right to left right to left left to right

b. right to left left to right right to left

c. left to right right to left left to right

d. left to right left to right right to left

e. left to right right to left right to left

19.

E0cell = -1.18- (-1.66) = 0.48 V

20.

Ecell = E0cell - (0.0591/n)log(Al^3+)^2 / (Zn^2+)^3

= 0.9-(0.0591/6)log(1.5^2/0.1^3)

= 0.867 v

b. 0.867 v

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