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Writing Balanced Redox Reaction from Cell Notation: Ni/Al Cell

CHEM-UJGBT5

Consider the following galvanic cell at $25 °C$:

$$\textrm{Ni}|\textrm{Ni}^{2+}(2.00\textrm{ M})||\textrm{Al}^{3+}(0.750 \textrm{ M})|\textrm{Al}$$

What is the balanced chemical equation that is represented by the cell notation above?

A

$\textrm{Al}(s) + 2.00\textrm{Ni}^{2+}(aq) \rightarrow \textrm{Ni}(s)+0.750\textrm{Al}^{3+}(aq)$

B

$2\textrm{Al}(s) + 3\textrm{Ni}^{2+}(aq) \rightarrow 3\textrm{Ni}(s)+2\textrm{Al}^{3+}(aq)$

C

$\textrm{Ni}(s)+0.750\textrm{Al}^{3+}(aq) \rightarrow \textrm{Al}(s) + 2.00\textrm{Ni}^{2+}(aq)$

D

$\textrm{Ni}(s)+ \textrm{Al}^{3+}(aq) \rightarrow \textrm{Al}(s) + \textrm{Ni}^{2+}(aq)$

E

$3\textrm{Ni}(s)+2\textrm{Al}^{3+}(aq) \rightarrow 2\textrm{Al}(s) + 3\textrm{Ni}^{2+}(aq)$