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Batteries Practice Test

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Q1

Imagine a galvanic cell which uses solid zinc and aqueous iron ions to produce a voltage.

$\small Zn(s) + $Fe^{2+}$(aq)\rightarrow $Zn^{2+}$(aq) + Fe(s)$

$\small $Zn^{2+}$ + $2e^{-}$\rightarrow Zn$ $\small \small E^ {\circ} = -0.76V$

$\small $Fe^{2+}$ + $2e^{-}$ \rightarrow Fe$ $\small $E^{\circ}$ = -0.44V$

The cell above resulted in a transfer of 0.05mol of electrons. The cell ran for four minutes at a constant voltage. What is the current of the cell?

$\small F=96,500$\frac{C}{mol}$$

You are charging your cell phone battery with your cell phone charger. What can you conclude about this process?

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