Calculate E_cell for an electrochemical cell based on the two half-reactions given below when the reaction occurs in an acidic aqueous solution in which the pH is buffered at 4.00 and [MnO₄-] = 1.80 M and [Fe²⁺] =0.0220 M.Use the smallest whole-number coefficients possible when
Balancing the overall reaction.

Question

Calculate E<sub>cell</sub> for an electrochemical cell based on the two half-reactions given below when the reaction occurs in an acidic aqueous solution in which the pH is buffered at 4.00 and [MnO<sub>4</sub>-] = 1.80 M and [Fe<sup>2+</sup>] =0.0220 M.Use the smallest whole-number coefficients possible when Balancing the overall reaction. A) (+2.10 V) B) (+0.964 V) C) (+1.21 V) D) (+1.86 V) E) (+2.38 V)

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The Answer of Calculate E_cell for an electrochemical cell based on the two half-reactions given below when the reaction occurs in an acidic aqueous solution in which the pH is buffered at 4.00 and [MnO₄-] = 1.80 M and [Fe²⁺] =0.0220 M.Use the smallest whole-number coefficients possible when Balancing the overall reaction.

Calculate Ecell for an Electrochemical Cell Based on the Two

Calculate E_cell for an Electrochemical Cell Based on the Two