The overall equation for the electrolysis of aluminium oxide is:

Chemistry

1 answer:

Alex Ar [27]2 years ago

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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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Answer:

$Molec_{\ H_{tot}}=1.206x10^{25}molec$

Explanation:

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In this case, taking into account that HCl has one molecule of hydrogen per mole of compound which weights 36.45 g/mol, we compute the number of molecules of hydrogen in hydrochloric acid by considering the given mass and the Avogadro's number:

$molec_{\ H}=3.65gHCl*\frac{1molHCl}{36.45gHCl} *\frac{1molH}{1molHCl}*\frac{6.022x10^{23}molec_\ H}{1molH} =6.03x10^{22}molec$

Now, from the 180 g of water, we see two hydrogen molecules per molecule of water, thus, by also using the Avogadro's number we compute the molecules of hydrogen in water:

$molec_{\ H}=180gH_2O*\frac{1molH_2O}{18gH_2O} *\frac{2molH}{1molH_2O}*\frac{6.022x10^{23}molec_\ H}{1molH} =1.20x10^{25}molec$