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Batteries Practice Test
•2 QuestionsQuestion
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Q1
Imagine a galvanic cell which uses solid zinc and aqueous iron ions to produce a voltage.
$\small Zn(s) + Fe^{2+}(aq)\rightarrow Zn^{2+}(aq) + Fe(s)$
$\small Zn^{2+} + 2e^{-}\rightarrow Zn$ 
$\small Fe^{2+} + 2e^{-} \rightarrow Fe$ 
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?
Imagine a galvanic cell which uses solid zinc and aqueous iron ions to produce a voltage.
$\small Zn(s) + Fe^{2+}(aq)\rightarrow Zn^{2+}(aq) + Fe(s)$
$\small Zn^{2+} + 2e^{-}\rightarrow Zn$
$\small Fe^{2+} + 2e^{-} \rightarrow Fe$
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?