Aluminum is mined as the mineral bauxite, which consists primarily of Al203 (alu

Question

Aluminum is mined as the mineral bauxite, which consists primarily of Al203 (alumina). The aluminum can be refined by heating the bauxite to drive off the oxygen: 2 Alzo, s a. How much aluminum is produced from 3.10 x 103 kg of Al203? Number Start by looking at the percent composition of 1.64 x 10 kg Al Al203 b. The oxygen produced in part (a) is allowed to react with carbon to produce carbon monoxide. Write a balanced equation describing the reaction of alumina with carbon ou need not include the states of matter in the balanced equation

Explanation / Answer

First Question -

Part (a) -

The balanced equation is -

2Al2O3 --> 4Al + 3O2

Now, use the above balanced equation to compare moles of reactants and products to determine the amount of reactants required and products formed.

3.10x10^3 kg = 3.10 x 10^6 g Al2O3
And, 3.10 x 10^6g / 102g/mole = 30392 moles

Therefore, quantity of aluminium produced = 30392 x (4Al / 2Al2O3) x 27g/mole x 1kg / 1000g = 1641.18 kg

(b) The requisite balanced equation is -

Al2O3 + 3 C -----> 2 Al + 3 CO

Second question -

The 0.210 g of solid Mg is Excess Reagent.

The gaseous O2 is Limiting Reagent.

The 0.248 g of solid MgO is actual yield.

The requisite equation is -

2Mg (s) + O2(g) -----------------------------> 2MgO

23.3 32 40.3

0.210 - 0.248

0.210/23.3 0.248/40.3

0.009 mol 0.00615 mol

From above, 0.009 mol of Mg should produce 0.009 mol of MgO

But, it produces only 0.00615 mol of MgO and it is due to limited availability of atmoshpheric oxygen.

So, percentage yield of this reaction = (0.00615 / 0.009)x100 = 68.33 %

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