Nernst Equation - Equilibrium Constant from Nernst Equation

Calculate the emf of the cell in which the following reaction takes place: 

\[\ce{Ni_{(s)} + 2Ag^+ (0.002 M) -> Ni^{2+} (0.160 M) + 2Ag_{(s)}}\]

Given that \[\ce{E^Θ_{cell}}\] = 1.05 V

For a cell reaction in involving a two electron change, the Stanford e. m. f of the cell is found to be 0.295 V at 25°C. The equilibrium constant of the reaction at 25°C will be

Under what condition is E_Cell = 0 or ∆_rG = 0?

Assertion: Current stops flowing when E_Cell = 0.

Reason: Equilibrium of the cell reaction is attained.

Write the Nernst equation for the cell reaction in the Daniel cell. How will the E_Cell be affected when concentration of Zn²⁺ ions is increased?

Can `E_(Cell)^Θ` or `∆_rG^Θ` for cell reaction ever be equal to zero?

Consider figure and answer the question to given below.

1. Redraw the diagram to show the direction of electron flow.
2. Is silver plate the anode or cathode?
3. What will happen if salt bridge is removed?
4. When will the cell stop functioning?
5. How will concentration of Zn²⁺ ions and Ag⁺ ions be affected when the cell functions?
6. How will the concentration of Zn²⁺ ions and Ag⁺ ions be affected after the cell becomes ‘dead’?

For the reaction H₂ + 1₂ ⇌ 2Hl, the relation between equilibrium constants Kp and Kc is