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Consider the cell Zn|Zn^(2+) (aq) (1.0M) ||Cu^(2+) (aq) (1.0M) |Cu The standard reduction potentials are +0.35 V for 2e+ Cu^(2+) (aq) to Cu and -0.763V for 2e+Zn^(2+) (aq) to Zn Write down the cell reaction. |
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Answer» SOLUTION :CELL REACTIONS are as FOLLOWS , RHS ELECTRODE `Cu^(2+) +2e=Cu` (reduction) LHS electrode `Zn=Zn^(2+)+2e` (oxidation) `therefore E_(cell)^@=E_(Ag^+,Ag)^@-E_(Cd^(2+),Cd)^@` `=0.80-(-0.40)` `=1.20` volts |
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