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maw [93]
2 years ago
8

n the 1990’s, the Boeing Co. developed a process for treating wastewater from electroplating and printed circuit board manufactu

ring. The central feature of the process was addition of scrap aluminum metal to an acidic solution containing dissolved copper ions. If the solution contained enough fluoride or chloride ions, a reaction proceeds in which the aluminum dissolved and the copper precipitated as metallic Cu(s), which could then be removed from the suspension by settling and/or filtration. The relevant reaction can be written as follows:233Cu2Al()3Cu()2Alss+++  +If a wastewater initially containing 300mg/L Cu2+and no dissolved aluminum is dosed with 100mg/L of Al scraps and the above reaction proceeds until equilibrium is reached, what will the final concentrations of Cu2+, Al3+, Cu(s), and Al(s) be?
Chemistry
1 answer:
scZoUnD [109]2 years ago
6 0

Answer:

Final concentrations:

Cu²⁺ = 0

Al³⁺ = 3.13 mmol/L = 84.51 mg/L

Cu = 4.7 mmol/L = 300 mg/L

Al = 0.57 mmol/L = 15.49 mg/L

Explanation:

2Al (s) + 3Cu²⁺ (aq) → 2Al³⁺ (aq) + 3Cu (s)

Al: 27 g/mol ∴ 100 mg = 3.7 mmol

Cu: 63.5 g/mol ∴ 300 mg = 4.7 mmol

3 mol Cu²⁺ _______ 2 mol Al

4.7 mmol Cu²⁺ _____ x

x = 3.13 mmol Al

4.7 mmol of Cu²⁺ will be consumed.

3.13 mmol of Al will be consumed.

4.7 mmol of Cu will be produced.

3.13 mmol of Al³⁺ will be produced.

0.57 mmol of Al will remain.

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Answer:

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3 years ago
Given the balanced equation below, calculate the moles of aluminum that are needed to react completely with 28.7 moles of FeO. Y
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Answer:

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Explanation:

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Moles of Al needed to react with FeO = ?

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Chemical equation:

2Al + 3FeO → 3Fe + Al₂O₃

Now we will compare the moles of Al with FeO.

                            FeO        :           Al

                             2            :            3

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