Asked by Stacy
                based on standard reduction potentials which metals would 
i) inhibit rusting
ii)promote rusting
My general statement is:
> If the reduction potential is higher it will inhibits rusting and if it is lower it will promote rusting
But im not sure because it doesn't make sense with Mg
            
        i) inhibit rusting
ii)promote rusting
My general statement is:
> If the reduction potential is higher it will inhibits rusting and if it is lower it will promote rusting
But im not sure because it doesn't make sense with Mg
Answers
                    Answered by
            Dr Jazz
            
    For a given reduction potential table, electron flow is from the more negative E-value to the more positive E-value. This would imply metals with a more negative E-value would undergo oxidation and the more positive E-value reduction. So, considering Zn => Zn^+2 + 2e (E = -0.76v) would be the reducing agent for Fe^+3 + 3e => Fe (E = -0.04v). As the Zn is the anode (undergoing oxidation) and the cathode (undergoing reduction) would indicate E-values that are more negative relative to  Fe reduction potential (assuming you are referring to Ferric Oxide rust) would inhibit rusting. Such is referred to as 'Cathodic Protection'; that is, one is trying to protect the metal at the cathode by connecting with a more negative E-value metal as the anode. The anode will disintegrate before the metal at the cathode. 
    
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