   Chapter 21, Problem 51PS

Chapter
Section
Textbook Problem

Aluminum sulfate is the most commercially important aluminum compound, after aluminium oxide and aluminum hydroxide. It is produced from the reaction of aluminum oxide and sulfuric acid. What masses (in kilograms) of aluminium oxide and sulfuric acid must be used to manufacture 1.00 kg of aluminum sulfate?

Interpretation Introduction

Interpretation:

The mass of aluminium oxide and sulfuric acid used to produce 1 kg of aluminium sulfate is to be predicted.

Concept introduction:

Aluminium sulfate is produced by the reaction of aluminium oxide and sulfuric acid. The formula for aluminium sulphate is Al2(SO4)3. It is an important commercial aluminium compound. The molar mass of aluminium sulphate is 342.15 g. The chemical reaction can be written as follows:

Al2O3(s)+3H2SO4(aq)Al2(SO4)3(s)+3H2O(l)

Explanation

The mass of aluminium oxide and sulfuric acid used to produce 1 kg of aluminium sulfate is calculated below.

Given:

The chemical reaction can be written as follows:

Al2O3(s)+3H2SO4(aq)Al2(SO4)3(s)+3H2O(l)

The molar mass of Al2(SO4)3 is 342.15 g.

The molar mass of Al2O3 is 101.96 g.

The molar mass of three moles of H2SO4 is 294.237 g.

Mass of Aluminium oxide used:

342.15 g of Al2(SO4)3 is manufactured from 101.96 g of Al2O3

1 g of Al2(SO4)3 is manufactured from 101.96 g342.15 g of Al2O3

1.00kg(1000g) of Al2(SO4)3 is manufactured from 101

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