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12 Dec 2019

When exposed to air, aluminum metal, Al, reacts with oxygen, O2, to produce a protective coating of aluminum oxide, Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here:

4Al+3O2→2Al2O3

In Part A, we saw that the theoretical yield of aluminum oxide is 1.30 mol . Calculate the percent yield if the actual yield of aluminum oxide is 0.910 mol .

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Casey Durgan
Casey DurganLv2
13 Dec 2019

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Related questions

4Al+3O2→2Al2O3

What is the theoretical yield of aluminum oxide if 1.40 mol of aluminum metal is exposed to 1.35 mol of oxygen?

9.Nickel, a common metal used in a variety of alloys, is purified via the Mond process to a very high (> 99.99%) purity. One of the steps in the Mond process involves the reaction of solid nickel with carbon monoxide to produce Ni(CO)4, as shown in the unbalanced equation below.

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How much carbon monoxide, in grams, is required to purify an impure sample containing 3.82 kg of nickel?

10.Thermite is a metal powder mixture used frequently in pyrotechnics and metal construction work. It is composed of highly powderized aluminum and iron(III) oxide and when ignited by a high temperature source (such as burning magnesium ribbon), it reacts according to the following equation.

Fe2O3(s) + 2 Al(s) → 2 Fe(l) + Al2O3(s)

What mass of powderized Al is required to completely react with 34.8 g Fe2O3?

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Determine the percent yield of the reaction, given that the actual yield of chromium chloride, CrCl3, was 29.5 g. (The molar mass of Cr2O3 is 152.00 g/mol and the molar mass of CrCl3 is 158.35 g/mol.)

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N2(g) + 3 H2(g) → 2 NH3(g)

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CHM111

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A) 10.0 g Ne

B) 10.0 g He

C) 10.0 g Ar

D) 10.0 g Kr

E) 10.0 g Mg

Q2. How many atoms are present in 0.23 moles of Calcium?

Q3. How many atoms are present in 5.6 mg of Silicon?

Q4. How many grams of iodine do 5.6 x 1025 atoms of iodine represent?

Q5. Balance the following Chemical Equations:

_____ CaC2(s) + _____H2O(l) ? _____ Ca(OH)2(aq) + _____ C2H2(g)

_____ P4O10 + _____ H2O? ______ H3PO4

___ C3H8O3 + ___ O2 ? ___ CO2 + ___ H2O

_____ C4H10(l) + _____ O2(g) ? _____ CO2(g) + _____ H2O(g)

___ Al + ___ N2 ? ___ Al2N3

___ NaN3 ? ___ Na + ___ N2

___ C3H5N3O9 ? ___ CO2 + ___ N2 + ___ H2O + ___ O2

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Q8. Determine the Empirical formula and Molecular formula of a compound that contains: 65.4% C, 9.15% H and 25.4% N by mass and has a molar mass of 220 g/mol.

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2KClO3 (s) ? 2 KCl + 3 O2 (g)

How many grams of O2 can be produced from 1.625 g of KClO3?

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If 6.25 moles of Fe react with 2.50 moles of Al2O3

Which reactant is the limiting reagent?

How many grams of Al are produced?

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2 AlCl3 (aq) + 3 H2SO4 (aq) ? Al2(SO4)3(aq) + 6 HCl (aq)

If 15.0 g of AlCl3was mixed with 25.0 g of H2SO4, which reactant is the limiting reagent?

Calculate the theoretical yield of Al2(SO4)3.

If only 18.63 g of Al2(SO4)3 was produced, what is the percent yield of Al2(SO4)3?

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