For a cell `Ag(s)|AgNO_(3)(0.01M)||AgNO_(3)(1.0M)|Ag(s)` (i). Calculate the e.m.f. of the cell at `25^(@)C` (ii). Write the net cell reaction. (iii).

Question

For a cell `Ag(s)|AgNO_(3)(0.01M)||AgNO_(3)(1.0M)|Ag(s)` (i). Calculate the e.m.f. of the cell at `25^(@)C` (ii). Write the net cell reaction. (iii).

For a cell `Ag(s)|AgNO_(3)(0.01M)||AgNO_(3)(1.0M)|Ag(s)`
(i). Calculate the e.m.f. of the cell at `25^(@)C`
(ii). Write the net cell reaction.
(iii). Will the cell generate e.m.f when two concentrations become equal?

Monjur Alahi

4 views

2025-01-04 04:42

1 Answers

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

Given: Electro chemical cell `Ag(s)|AgNO_(4)(0.01M)||AgNO_(3)(1.0M)|Ag(s)`
Asked: (i). To write the net cell reaction
(ii). To calculate the e.m.f of the cell at `25^(@)C`?
(iii). To calculate the e.m.f when two concentration become equal?
Formula used: `E_(cell)=E_(cell)^(@)-(0.0591)/(n)log((["product"])/(["reactant"]))` ltbr. Explanation `E_(cell)^(@)=` standard e.m.f of cell
`E_(cell)=e.m.f` of cell
Substitution and calculation:
(i). `E_(cell)=(0.0591)/(1)log(([Ag^(+)(conc.)])/([Ag^(+)(dil.)]))`
`E_(cell)=0.0591xxlog((1)/(0.01))=0.0591log100=0.0591xx2=0.1182V`
(ii). `Ag^(+)(1.0M)+Ag(s)toAg^(+)(0.01M)+Ag(s)`
(iii). No, e.m.f. will becomes zero.