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  • $\begingroup$ Thank you that is very helpful. In regard to the nickel electrodes would I be correct in assuming that nickel, like aluminum, also forms this instantaneous oxide layer? Also, would zinc then take longer to form this oxidation layer or is there some other explanation as to why its value matched the theoretical? $\endgroup$
    – John
    Commented Jan 11, 2021 at 1:26
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    $\begingroup$ @John Purely by the standard redox potential for $\ce{Ni(s)/Ni^2+(aq)}$, nickel should be quite reactive. The fact that it is not and is used in corrosion resistent alloys or metal platings says something. $\ce{ZnO}$ is probably not so compact and is quite soluble in acidic solutions. Note also that some standard redox potentials are more or less just theoretical equivalents of related standard reaction Gibbs energy and cannot be ( or just with difficulties ) directly measured, at least in simple scenarios. I have once seen redox potential for C/CH4 and would like to see its measurement. $\endgroup$
    – Poutnik
    Commented Jan 11, 2021 at 7:31
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    $\begingroup$ The operation is forbidden by law? I'm surprised to hear that it's illegal to mix two chemicals. I would expect that it's legal to mix them but then the law would be very picky about how you dispose of the mercury compounds - including the mercury dissolved in the aluminium, if it does that. $\endgroup$
    – Stack Exchange Supports Israel
    Commented Jan 11, 2021 at 16:25
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    $\begingroup$ @User253751 In my country you cannot use mercury in chemistry lectures and in the laboratory. $\endgroup$
    – Maurice
    Commented Jan 11, 2021 at 19:34
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    $\begingroup$ @user253751 - many things are banned in school labs but not others. $\endgroup$
    – Michael Harvey
    Commented Jan 12, 2021 at 6:59