Question #c11d7

1 Answer
Mar 4, 2017

Answer:

#E_"cell" = 2.175V#

Explanation:

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#