Standard electrode potentials are given as, `E_(Cu^(2+)//Cd)^(@)=0.34" V " " and " E_(Ag^(+)//Ag)^(@)=0.80" V "` Calculate the cell potential, E for c

Question

Standard electrode potentials are given as, `E_(Cu^(2+)//Cd)^(@)=0.34" V " " and " E_(Ag^(+)//Ag)^(@)=0.80" V "` Calculate the cell potential, E for c

Standard electrode potentials are given as,
`E_(Cu^(2+)//Cd)^(@)=0.34" V " " and " E_(Ag^(+)//Ag)^(@)=0.80" V "`
Calculate the cell potential, E for cell containing 0.100 M `Ag^(+)` and 4.00 M `Cu^(2+)` at `25^(@)C`.

Monjur Alahi

7 views

2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

Correct Answer - 0.3831 V
Cell reaction : `Cu(s)+2Ag^(+)(0.1" M") to Cu^(2+)(4.0" M")+2Ag(s)`
`E_(cell)=E_(cell)^(@)-(0.0591)/(n)"log"([Cu^(2+)])/([Ag^(+)]^(2))=[(0.8)-(+0.34)]-(0.0591)/(2)"log"((4.0))/((0.1)^(2))`
`=0.46-0.02955 log 400=0.46-0.02955xx2.6021=0.3831" V "`

7 views Answered 2023-02-05 15:29