Chapter 14.4, Problem 8TY

Interpretation Introduction

Interpretation:

Whether the direction of reaction remains the same in the given cell has to be given.

Concept Introduction:

For complete cell, the Nernst equation is: ${\text{E = E}}^{\text{+}}-{\text{ E}}^{-}$

Steps for writing net cell reaction and calculating its voltage:

• Find $\text{E°}$ of the half-cells by writing reduction half-reactions. The half-reactions has to be multiplies by necessary numerals so as to get same number of electrons.
• Write Nernst equation for right half-cell. This will be ${\text{E}}_{+}$
• Write Nernst equation for left half-cell. This will be ${\text{E}}_{-}$
• The subtraction of these two voltages gives the net cell voltage
• Subtract left half-reaction from right half-reaction and write the net cell reaction.
• When the calculated ${\text{E = E}}^{\text{+}}-{\text{ E}}^{-}$ is positive, the flow of electrons will be from left-hand electrode to right-hand electrode and when it is negative, the direction will be opposite.

To Give: Whether the direction of reaction remains the same in the given cell