Question #c11d7

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Answer 1 · 2017-03-04T10:12:40

$E_"cell" = 2.175V$

First write the balanced equations

$Zn + Cl_2 → 2Cl^-)+ Zn^(2+)$

$Zn rarr Zn^(2+) + 2e^-) E^o "red" = -0.7618V$

$E^o "ox" = -( E^o "red")$

Therefore $E^o "oxn" = +0.7618V$

$Cl_2 + 2e^-) → 2Cl^-) E^o"red" = 1.36V$

$E^ocell = E^o"red" + E^o"oxn"$

$E^ocell = 1.36 V + 0.76 V = 2.12 V$

Now solve for Nernst equation

$Q = (0.15)(0.30)^2$

$Ecell = 2.12 V - {("0.0592 V"/2)log(0.15)(0.30)^2}$

$2.175 V$

$E_"cell "= 2.175V$