Question

1)What element is being oxidized in the following redox reaction?

Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^-

1B) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in frot of H+ and Fe3+ in the balance reaction?

Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+

1C) determine the cell notation for the redox reaction given below. [hint: remember sometimes inert electrodes are used.

3 Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2 Fe 3+ (aq)

Answer 1

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^-

oxidation = species that losses electrons...

from the previous reaction

Cr goes from +3 in Cr(OH)4- to +6 in CrO4-2 ... This implies that +3 to +6 has a 3 electron charge loss... that is, it is being oxidized

1B) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in frot of H+ and Fe3+ in the balance reaction? Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+

split reaction:

Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+

MnO4- = Mn+2

Fe+2 = Fe+3

balance O

MnO4- = Mn+2 + 4H2O

Fe+2 = Fe+3

balance H

8H+ + MnO4- = Mn+2 + 4H2O

Fe+2 = Fe+3

balance charge

5e- + 8H+ + MnO4- = Mn+2 + 4H2O

Fe+2 = Fe+3 + 2e-

balance

10e- + 6H+ + 2MnO4- = 2Mn+2 + 8H2O

5Fe+2 = 5Fe+3 + 10e-

add all

5Fe+2 + 10e- + 6H+ + 2MnO4- = 2Mn+2 + 8H2O +  5Fe+3 + 10e-

the coefficient of H+ is 6;

coefficient of Fe3+ is 5

1C) determine the cell notation for the redox reaction given below. [hint: remember sometimes inert electrodes are used. 3 Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2 Fe 3+ (aq)

Cell notation:

oxidation // Reduction

Fe(s)/Fe3+ // Cl2(g) / Cl-(aq)