# The Nernst Equation Write the Nernst equation2 for the reaction Cu2+ (aq) + Zn (s)  Zn2+ (aq) + Cu (s) Let activity of Cu2+ equal to 1 and change the activity of Zn2+ such that Q is in the range  0.001 to +0.001. Select different values of Q and for each calculate Ecell. Plot E_"cell" -E_"cell" ^ө vs ln Q. What is the effect of Q (that is the activity) on E_"cell" -E_"cell" ^ө ? Is the effect the same at higher and lower values of Q? what is the largest value of the absolute difference between cell potential and standard cell potential, |E_"cell" -E_"cell" ^ө |? What do you expect the graph will look like for different number of electron transferred ( )? And why?

Question

Part B: The Nernst Equation
Write the Nernst equation2 for the reaction Cu2+ (aq) + Zn (s)  Zn2+ (aq) + Cu (s)
Let activity of Cu2+ equal to 1 and change the activity of Zn2+ such that Q is in the range  0.001 to +0.001. Select different values of Q and for each calculate Ecell. Plot E_"cell" -E_"cell" ^ө vs ln Q. What is the effect of Q (that is the activity) on E_"cell" -E_"cell" ^ө ? Is the effect the same at higher and lower values of Q? what is the largest value of the absolute difference between cell potential and standard cell potential, |E_"cell" -E_"cell" ^ө |? What do you expect the graph will look like for different number of electron transferred ( )? And why?