How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A

Question

Quizplus · Accepted Answer

First, we need to balance the equation: 2 Al^{3 + 3} → 2 Al + 3 S1U1P4 From the equation, 2 moles of Al^{3 produces 2 moles of Al, which has a molar mass of 26.98 g/mol. This means that 2 moles of Al has a mass of 53.96 g.

Using the formula,

mass = (current × time × molar mass) / (n × F)

where n is the number of electrons involved in the reaction (in this case, 6, since each Al3+ ion requires 3 electrons to reduce to Al) and F is Faraday's constant (96500 C/mol), we can solve for time:

78 g = (2.0 A × time × 26.98 g/mol) / (6 × 96500 C/mol)

Solving for time, we get:

time = 116 hours or 6947 minutes

Therefore, the answer is D: 116 h.}

How Long Will It Take to Produce 78 G of Al