Consider two cells, the first with Al and Ag electrodes and the second with Zn and Ni electrodes, each in 1.00 M solutions of their ions. If connected as voltaic cells in series, which two metals are plated, and what is the total potential, E ∘ ? Which two metals are plated?

a. Al ( s )

b. Ag ( s )

c. Zn ( s )

d. Ni ( s )

E ∘ =

b. Ag ( s )

d. Ni ( s )

 = 2.97 V

Explanation:

The reduction potentials for the given four (4) electrodes are:

In the first cell:

In the second cell:

Since the cells are connected in series :

Thus; Metal plated in the first  cell = Ag

Metal plated in the second cell = Ni

The total potential =

= (0.80 + 1.66 ) V - (0.25 +0.76 ) V

= 2.97 V

given the reactants, h2so4 and koh, we are asked to determine the product(s) of the reaction. since h2so4 is an acid and koh is a base. this is a neutralization reaction, thus, the products are salt and water. 

so, h+ from h2so4 will react with oh- from koh forming h2o. k+ will also react with so4 2- forming k2so4. therefore, the balanced reaction will be:

h2so4 + 2koh > k2so4 + 2h2o

explanation: