Zinc is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effectis to reverse the oxidation of iron to iron (II) by causing zinc to oxidize to the zinc ion. Calculate the voltage for this reaction if it takes place under standard conditions.
Zinc is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effectis to reverse the oxidation of iron to iron (II) by causing zinc to oxidize to the zinc ion. Calculate the voltage for this reaction if it takes place under standard conditions.
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 27E: Determine the overall reaction and its standard cell potential at 25 C for the reaction involving...
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Zinc is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effectis to reverse the oxidation of iron to iron (II) by causing zinc to oxidize to the zinc ion. Calculate the voltage for this reaction if it takes place under standard conditions.
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