a current of 5.25 a is applied to the aluminum sulfate solution for 112 minutes. what mass of al is plated…

Explanation:

Step1: Convert time to seconds

$112\ \text{min} \times 60\ \text{s/min} = 6720\ \text{s}$

Step2: Calculate total charge (Q=I×t)

$Q = 5.25\ \text{A} \times 6720\ \text{s} = 35280\ \text{C}$

Step3: Find moles of electrons

Molar charge of 1 mol $e^- = 96485\ \text{C/mol}$ $\text{Moles of } e^- = \frac{35280\ \text{C}}{96485\ \text{C/mol}} \approx 0.3656\ \text{mol}$

Step4: Relate to moles of Al

3 mol $e^-$ produce 1 mol Al $\text{Moles of Al} = \frac{0.3656\ \text{mol}}{3} \approx 0.1219\ \text{mol}$

Step5: Calculate mass of Al

Molar mass of Al = $26.98\ \text{g/mol}$ $\text{Mass of Al} = 0.1219\ \text{mol} \times 26.98\ \text{g/mol}$

Answer:

3.29 g Al