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Use the table of standard reduction potentials provided below to analyze the following reaction:

$$2 {\textrm{H}_2}_{(g)} + {\textrm{O}_2}_{(g)} \rightarrow 2 {\textrm{H}_2\textrm{O}}_{(l)}$$

In a hydrogen-oxygen fuel cell, energy is produced by the overall reaction represented above.

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(A) When the fuel cell operates at $25˚C$ and $1.00 \textrm{ atm}$ for $46.0 \textrm{ minutes}$, $0.0432 \textrm{ mol}$ of ${\textrm{O}_2}_{(g)}$ are consumed. How many moles of ${\textrm{H}_2}_{(g)}$ are consumed during this time period?
Select Option $0.0216\ mol $$0.0432\ mol $$0.0864\ mol$$0.173\ mol $
(B) Given that the fuel cell reaction takes place in an acidic medium, what is the value of the standard potential, $E˚$, of the cell?
Select Option $-1.23\ V $$ -0.74\ V$$0.00\ V $$0.49\ V$$0.74\ V$$1.23\ V$
(C) What is the charge, in coulombs, that passes through the cell during the $46.0\ \text{minutes}$ of operation as described in part (A)?
Select Option $6.04\ C $$2760\ C$$4180\ C $$8350\ C$ $16700\ C$
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