# Problem: Exercise 46. Give the balanced cell equation and determine E° for the galvanic cells based on the following half-reactions. Standard reduction potentials are found in Table 17‑1.a. Cr2O72- + 14H+ + 6e- → 2Cr 3+ + 7H2O    H2O2 + 2H+ + 2e- → 2H2Ob. 2H + + 2e- → H2    Al 3+ + 3e- → AlCalculate the maximum amount of work that can be obtained from the galvanic cells at standard conditions in Exercise 46.

###### FREE Expert Solution

Recall:

Lose               Gain
Electron         Electrons
Oxidation       Reduction

cathode → reduction → oxidation number decreases

anode → oxidation → oxidation number increases

For ions: charge of the ion = oxidation number
For neutral atoms/compound: oxidation number = 0

A.

Cr2O72- + 14H+ + 6e- → 2Cr 3+ + 7H2O

[H2O2 + 2H+ + 2e- → 2H2O]×3

98% (366 ratings)
###### Problem Details

Exercise 46. Give the balanced cell equation and determine E° for the galvanic cells based on the following half-reactions. Standard reduction potentials are found in Table 17‑1.

a. Cr2O72- + 14H+ + 6e- → 2Cr 3+ + 7H2O
H2O2 + 2H+ + 2e- → 2H2O

b. 2H + + 2e- → H2
Al 3+ + 3e- → Al

Calculate the maximum amount of work that can be obtained from the galvanic cells at standard conditions in Exercise 46.