Given the following data: Fe2+(aq) + 2e- ( Fe(s) E0red = -0.44 v , Cr3+(aq) + e- ( Cr2+(aq) E0red = -0.407 v a) What is the spontaneous cell reaction when a voltaic cell is constructed using these two half- reactions?

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Answer 1 · 2018-04-22T16:35:16

#Fe(s)+2Cr^(3+)(aq)->Fe^(2+)+2Cr^(2+)(aq)#

In an voltaic cell, the #V# should be positive, so:
#Fe(s)# must be oxidized:# 0.44 V#

#Cr^(3+)#must be reduced: #-0.407 V#

Net Cell potential: #0.44 V-0.407V= 0.033 V#

Here's your net reaction:
#Fe(s)+2Cr^(3+)(aq)+cancel(2e^-)->Fe^(2+)+2Cr^(2+)(aq)+cancel(2e^-)#