Question

For a cell Ag/AgNO3(0.01M)//AgNO3(1.0M)/Ag i) Calculate the emf of the cell at 298K Ii) Write the Nernst cell reaction iii) Will the cell generate emf, when two concentration became equal

Answer 1

Answer:

THE ANSWER IS 0.1182V

Explanation:

For a cell

Ag/AgNO3(0.01M)//AgNO3(1.0M)/Ag

E°Cell = E°Ag⁺/Ag-E°Ag⁺/Ag = 0V

USING NERNST EQUATION,

ECell = E°Cell - 0.0591/n log[Ag⁺]/[Ag⁺]

ECell = 0 - 0.0591/1 log [0.01]/[1.0]

ECell =  -0.0591*(-2)

ECell = 0.1182V

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Answer 2

Answer:

0

Explanation:

When the two conc become equal then log[product]/[reactant] = log 1 which is equal to 0 and the Eo is already 0 so there will be no emf when the conc is zero in a conc cell]