Question

Consider the following BALANCED half-reactions at 25 °C: MnO4- + 8H+ + 5e- ? Mn2+ + 4H2O E° = +1.51 V ClO3- + 6H+ + 6e- ? Cl- + 3H2O E° = +1.45 V Calculate the standard Gibbs energy change ?G° for the spontaneous redox reaction based on the above half-reactions. (A) -85000 kJ (B) -1700 kJ (C) -170 kJ (D) -35 kJ (E) -29 kJ

          Consider the following BALANCED half-reactions at 25 °C:
MnO4- + 8H+ + 5e- ? Mn2+ + 4H2O E° = +1.51 V
ClO3- + 6H+ + 6e- ? Cl- + 3H2O E° = +1.45 V
Calculate the standard Gibbs energy change ?G° for the spontaneous redox
reaction based on the above half-reactions.
(A) -85000 kJ
(B) -1700 kJ
(C) -170 kJ
(D) -35 kJ
(E) -29 kJ

Consider the following BALANCED half-reactions at 25 °C:
MnO4- + 8H+ + 5e- ? Mn2+ + 4H2O E° = +1.51 V
ClO3- + 6H+ + 6e- ? Cl- + 3H2O E° = +1.45 V
Calculate the standard Gibbs energy change ?G° for the spontaneous redox
reaction based on the above half-reactions.
(A) -85000 kJ
(B) -1700 kJ
(C) -170 kJ
(D) -35 kJ
(E) -29 kJ

Added by Michael J.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

09/05/2023

Step 1

MnO4- + 8H+ + 5e- -> Mn2+ + 4H2O (E° = +1.51 V) 2ClO- + 6H+ + 6e- -> 2Cl- + 3H2O (E° = +1.45 V) To balance the electrons, we need to multiply the first half-reaction by 6 and the second half-reaction by 5: 6(MnO4- + 8H+ + 5e- -> Mn2+ + 4H2O) (E° = +1.51 Show more…

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Consider the following BALANCED half-reactions at 25 °C: MnO4- + 8H+ + 5e- ⇌ Mn2+ + 4H2O E° = +1.51 V ClO3- + 6H+ + 6e- ⇌ Cl- + 3H2O E° = +1.45 V Calculate the standard Gibbs energy change ΔG° for the spontaneous redox reaction based on the above half-reactions: (A) -85000 kJ (B) -1700 kJ (C) -170 kJ (D) -35 kJ (E) -29 kJ