QuestionJune 29, 2025

How many hours would it take to reduce one mole of Al^+3 to aluminum using a current of 22.2 Amps? A) 13020 hours B) 3.6 hours C) 0.22 hours D) 217 hours

How many hours would it take to reduce one mole of Al^+3 to aluminum using a current of 22.2 Amps? A) 13020 hours B) 3.6 hours C) 0.22 hours D) 217 hours
How many hours would it take
to reduce one mole of Al^+3 to
aluminum using a current of
22.2 Amps?
A) 13020 hours
B) 3.6 hours
C) 0.22 hours
D) 217 hours

Solution
4.1(291 votes)

Answer

B) 3.6 hours Explanation 1. Determine the charge needed The reduction of Al^{+3} to Al requires 3 moles of electrons per mole of aluminum. **Faraday's constant** is used to find the total charge: Q = n \cdot F, where n = 3 moles and F = 96485 \, C/mol. So, Q = 3 \times 96485 = 289455 \, C. 2. Calculate time using current Use the formula **t = \frac{Q}{I}**, where I = 22.2 \, A. Thus, t = \frac{289455}{22.2} = 13035.36 \, s. 3. Convert seconds to hours Convert seconds to hours: \frac{13035.36}{3600} \approx 3.62 \, \text{hours}.

Explanation

1. Determine the charge needed<br /> The reduction of $Al^{+3}$ to Al requires 3 moles of electrons per mole of aluminum. **Faraday's constant** is used to find the total charge: $Q = n \cdot F$, where $n = 3$ moles and $F = 96485 \, C/mol$. So, $Q = 3 \times 96485 = 289455 \, C$.<br />2. Calculate time using current<br /> Use the formula **$t = \frac{Q}{I}$**, where $I = 22.2 \, A$. Thus, $t = \frac{289455}{22.2} = 13035.36 \, s$.<br />3. Convert seconds to hours<br /> Convert seconds to hours: $\frac{13035.36}{3600} \approx 3.62 \, \text{hours}$.
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