Question

Use the appropriate standard reduction potentials below to determine the equilibrium constant at 271 K for the following reaction under acidic conditions. 4H?(aq) + MnO?(s) + 2Fe²?(aq) ? Mn²?(aq) + 2Fe³?(aq) + 2H?O(l) Standard reduction potentials: MnO?(s) + 4H?(aq) + 2e? ? Mn²?(aq) + 2H?O(l) E° = 1.23 V Fe³?(aq) + e? ? Fe²?(aq) E° = 0.770 V

          Use the appropriate standard reduction potentials below to determine the equilibrium constant at 271 K for the following reaction under acidic conditions.

4H?(aq) + MnO?(s) + 2Fe²?(aq) ? Mn²?(aq) + 2Fe³?(aq) + 2H?O(l)

Standard reduction potentials:
MnO?(s) + 4H?(aq) + 2e? ? Mn²?(aq) + 2H?O(l) E° = 1.23 V
Fe³?(aq) + e? ? Fe²?(aq) E° = 0.770 V

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Use the appropriate standard reduction potentials below to determine the equilibrium constant at 271 K for the following reaction under acidic conditions.

4H?(aq) + MnO?(s) + 2Fe²?(aq) ? Mn²?(aq) + 2Fe³?(aq) + 2H?O(l)

Standard reduction potentials:
MnO?(s) + 4H?(aq) + 2e? ? Mn²?(aq) + 2H?O(l) E° = 1.23 V
Fe³?(aq) + e? ? Fe²?(aq) E° = 0.770 V

Added by Christopher A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

12/11/2022

Step 1

The first half-reaction is already balanced. The second half-reaction needs to be reversed and multiplied by 2 to match the overall reaction: 2Fe3+(aq) → 2Fe2+(aq) + 2e- E° = -1.23 V Show more…

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Use the appropriate standard reduction potentials below to determine the equilibrium constant at 271 K for the following reaction under acidic conditions: 4H+(aq) + MnO2(s) + 2Fe2+(aq) → Mn2+(aq) + 2Fe3+(aq) + 2H2O(l) Standard reduction potentials: MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(l) E° = 1.23 V Fe3+(aq) + e- → Fe2+(aq) E° = 0.770 V

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