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2 years ago

The overall equation for the electrolysis of aluminium oxide is:

Chemistry

1 answer:

Alex Ar [27]2 years ago

6 0

941539.2 g of mass of oxygen is produced when 2000 kg of aluminium oxide is completely electrolysed.

<h3>What is electrolysis?</h3>

Electrolysis is the process by which electric current is passed through a substance to effect a chemical change.

The mass of aluminium oxide Al₂O₃ = 2000 kg = 2000 000 g

Molar mass of Al₂O₃ = 101.96 g/mol

no of moles = $\frac{mass }{ molar \;mass}$

no of moles of Al₂O₃ = $\frac{2000 000 g}{101.96 g/mol}$

no of moles of Al₂O₃ = 19615.4 mol

From the reaction:

4Al + 3O₂ ⇒ Al₂O₃

To determine the moles of O₂ in Al₂O₃:

Then;

19615.4 mol X $\frac{3}{2}$ mol of O₂ = 29423.1

The mass of oxygen now = 29423.1 × 32 g

= 941539.2 g

Hence, 941539.2 g of mass of oxygen is produced when 2000 kg of aluminium oxide is completely electrolysed.

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Write a balanced half-reaction for the reduction of permanganate ion mno−4 to solid manganese dioxide mno2 in acidic aqueous sol

Svetlanka [38]

The half-reaction includes either the reduction or the oxidation reaction of the redox reactions. In acidic solution permanganate ion will react with hydrogen ion to yield manganese ion and water.

<h3>What are Redox reactions?</h3>

Redox or oxidation-reduction reactions are the chemical reactions in which the oxidation and the reduction of the chemical species occur simultaneously.

Permanganate (VII) ion is a strong oxidizing agent and gets easily reduced to manganese ion in presence of the hydrogen ion in an acidic solution.

The balanced half-reaction for reduction is shown as,

$\rm MnO_{4}^{-} \; (aq)+ 8H^{+} \; (aq)+ 5e^{-} \rightarrow Mn^{2+} \; (aq)+ 4H_{2}O \; (l)$

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2 years ago

PLEASE HELP!!

Mandarinka [93]

Answer:

a. 211.7

Explanation:

Iron Pyrite reacts with Oxygen to produce Iron (II) Oxide and Sulphur (IV) Oxide.

The equation is as follows:

4FeS₂₍s₎ + 11O₂₍g₎ → 2Fe₂O₃₍s₎ + 8SO₂₍g₎

From the equation, 4 moles of FeS₂ produce 8 moles of SO₂.

Therefore the reaction ratio is 4:8 or 1:2

198.20 grams of FeS₂ into moles is calculated as follows:

Moles= Mass/RMM

RMM of FeS₂ is 119.9750g/mol.

Number of moles = 198.20/119.9750g/mol

=1.652 moles of FeS₂

The reaction ratio of FeS₂ to SO₂ produced is 1:2

Thus SO₂ produced = 1.652 moles×2/1=3.304 moles

The mass of SO₂ produced =Moles ×RMM

=3.304 moles ×64.0638 g/mol

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