own below is a galvanic cell with anode compartment b comaining anode a and cath

Question

own below is a galvanic cell with anode compartment b comaining anode a and cathode compartment d containing cathode c. Electrons flow through wire f, ions flow through salt bridge e, and the cell potential is read using voltmeter g This galvanic cell uses the reaction: Cu(s)+2 Ag (ag)-2 Ag(s)+ Cu2+(aq) 6) The initial concentrations of Ag (ae) and Cu2+(aq) are both 1.0 M. What will happen to the cell 6) voltage if 5.0 M AgNO3 is added to the compartment containing the 1.0 M Ag (aq)? The cell voltage will A) decrease C) remain the same. B) increase. D) can't tell from the information given

Explanation / Answer

Answer:

if we add 5M AgNO3 in a compartment which containing 1 M Ag+ that means we are increasing the concentration of an electrolyte. Cation and anion present in this compartment also increase, thus cell potential also increase.

In a mathematical way,

we know that Nernst equation

Ecell = Eocell (0.0257/n) lnQ

where Q = [Cu+2] / [Ag+]

so if we increase  [Ag+] then vaule of Q decrease that means 'InQ' value also got decrease . hence, the value of cell potential increase.

B option is correct

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