If the [Zn?] = 2.0 M and [A1+] = 0.50 M, this would be a non-standard cell. Using the relationships AG = - nF and AG° =

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If The Zn 2 0 M And A1 0 50 M This Would Be A Non Standard Cell Using The Relationships Ag Nf And Ag 1 (51.19 KiB) Viewed 7 times

If the [Zn?] = 2.0 M and [A1+] = 0.50 M, this would be a non-standard cell. Using the relationships AG = - nF and AG° = -nFº we can come up with an equation to calculate non-standard cell potentials, the Nernst equation {=&º- RT In Q =<- RT log Q {=&° -0.0592 log Q nF where n = #moles of electrons in the balanced half-reactions F = Faradays constant 296,485 C/mol e nF Q = reaction quotient, [products/ [reactants] 3. Calculate non-standard cell potential (E) at 298 K when the [Zn2+] = 2.0 M and [A14] = 0.50 M. a) Q = b) &° = c) n = d) = 4. Calculate AG and AGº and discuss the difference in the work being done in terms of [products) and [reactants] a) Agº b) AG = 5. What is the effect on the cell potential, &; if a student doubles the size(mass) of the aluminum electrode, explain? 6. What is the effect on the cell potential, &; if a student added an additional 500 mL of water to the cathode, assuming there was 1.0 L of the solution to begin with, explain?