There is an electrolytic cell in which Mn2+ is reduced to Mn and Sn is oxidized to Sn2+. A. Write an equation for the half-reaction occurring at each electrode. Express your answers as chemical equations separated by a comma. Identify all of the phases in your answer.
B. What minimum voltage is necessary to drive the reaction? Vmin =

See explanation

Explanation:

Anode;

Sn(s) > Sn^2+(aq) + 2e

Cathode;

Mn^2+(aq) + 2e > Mn(s)

The minimum voltage required to drive the reaction is the cell voltage. The cell voltage is obtained from;

E°cell= E°cathode - E°anode

E°cell= -1.19 - (-0.14)

E°cell= -1.05 V

i believe it is c.) 1575 j.

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b