Concept explainers
Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.
Concept introduction: Corrosion is a natural process. The destruction of metals by
Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.
The loss of electrons is called oxidation whereas the gain of electrons is called reduction.
In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.
The copper is oxidized by air in seawater. The
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Chemistry & Chemical Reactivity
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- A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s)+H2O(l)+2eHg(l)+2OH(aq)Zn(s)+2OH(aq)Zn(OH)2(s)+2e Which half-reaction occurs at the anode and which occurs at the cathode? What is the overall cell reaction?arrow_forwardWhy would a sacrificial anode made of lithium metal be a bad choice despite its ELi+/Li=2.07V, which appears to be able to protect all the other metals listed in the standard reduction potential table?arrow_forwardWhich of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.arrow_forward
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