AP Chemistry
9.11 Electrolysis and Faraday’s Law
A student performs an electrolysis experiment to decompose water. A constant current of \(1.93 \text{ A}\) is passed through an acidified aqueous solution for \(2{,}000 \text{ s}\). The oxidation half-reaction occurring at the anode is shown below.
\[ 2\text{H}_2\text{O}(l) \rightarrow \text{O}_2(g) + 4\text{H}^+(aq) + 4e^- \]
Assuming ideal gas behavior, what volume of \(\text{O}_2(g)\) is produced at STP (\(0^\circ\text{C}\) and \(1.0 \text{ atm}\))? (Faraday's constant: \(F = 96{,}500 \text{ C/mol } e^-\); molar volume of an ideal gas at STP \(= 22.4 \text{ L/mol}\).)
\[ 2\text{H}_2\text{O}(l) \rightarrow \text{O}_2(g) + 4\text{H}^+(aq) + 4e^- \]
Assuming ideal gas behavior, what volume of \(\text{O}_2(g)\) is produced at STP (\(0^\circ\text{C}\) and \(1.0 \text{ atm}\))? (Faraday's constant: \(F = 96{,}500 \text{ C/mol } e^-\); molar volume of an ideal gas at STP \(= 22.4 \text{ L/mol}\).)
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