Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or)E=E^@ - (0.0591)/(n) log Q E^@= Standard potential and 'Q' is the reaction quotient. Which cell has least potential ?

Nernst equation gives the variation of potential of an electrode based

1.	Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or)E=E^@ - (0.0591)/(n) log Q E^@= Standard potential and 'Q' is the reaction quotient. Which cell has least potential ?
Answer» `ZN// UNDERSET(1M)(Zn^(+2))// underset(1M)(Cu^(+2))//Cu` `Zn// underset(0.1M)(Zn^(+2))// // underset(0.1M)(Cu^(+2))// Cu` `Zn // underset(0.1M)(Zn^(+2))// underset(1M)(Cu^(+2))// Cu` `Zn// underset(1M)(Zn^(+2))// underset(0.1M)(Cu^(+2))// Cu` Solution :`E_("cell") = E_("cell")^(0) + (0.0591)/(n) LOG "([Cu^(+2)])/([Zn^(+2)])` ` [Cu^(+2)] uarrE_("cell") uarr ` ` [Cu^(+2)] darr E_("cell")darr` Metallurgy , Refer Ellingham Diagram According to this graph lower line metal reduce upper line metal