Question

Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:

(textCu^2+ (textaq) + 2textFe^2+ (textaq) rightarrow textCu (texts) + 2textFe^3+ (textaq)).

Which of the following expressions correctly represents the cell potential ((E^˚_textcell)) and the equilibrium constant ((K)) for the given reaction at 298 K?

A) (E^˚_textcell = E^˚_textcathode - E^˚_textanode), (K = textFe^3+^2textCu^2+textFe^2+^2)
B) (E^˚_textcell = E^˚_textanode - E^˚_textcathode), (K = textCu^2+textFe^2+^2textFe^3+^2)
C) (E^˚_textcell = E^˚_textanode + E^˚_textcathode), (K = textFe^3+^2textCu^2+textFe^2+^2)
D) (E^˚_textcell = E^˚_textcathode + E^˚_textanode), (K = textFe^3+textCu^2+^2textFe^2+^2)

Answer 1

The correct expressions to represent the cell potential and the equilibrium constant for the given reaction at 298 K are: (E^˚_cell = E^˚_cathode - E^˚_anode), (K = [Fe^3+]^2/[Cu^2+]^2[Fe^2+]^2)

Step-by-step explanation:

The correct expressions to represent the cell potential (E^˚_cell) and the equilibrium constant (K) for the given reaction at 298 K are:

A) (E^˚_cell = E^˚_cathode - E^˚_anode), (K = [Fe^3+]^2/[Cu^2+]^2[Fe^2+]^2)