   Chapter 4.4, Problem 4.3CYU

Chapter
Section
Textbook Problem

One method for determining the purity of a sample of titanium(IV) oxide, TiO2, an important industrial chemical, is to react the sample with bromine trifluoride.3 TiO2(s) + 4 BrF3(ℓ) → 3 TiF4(s) + 2 Br2(ℓ) + 3 O2 (g)This reaction is known to occur completely and quantitatively. That is. all of the oxygen in TiO2, is evolved as O2 Suppose 2.367 g of a TiO2-containng sample evolves 0.143 g O2. What is the mass percent of TiO2 in the sample?

Interpretation Introduction

Interpretation:

The mass percentage of TiO2 in the given sample of compound should be determined.

Concept introduction:

• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• Mass percentage of reacted mass in the original sample is the ratio of mass of substance reacted to mass of whole sample taken.
• Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Balanced chemical equation for the given reaction is,

3TiO2(s)+4BrF3(l)3TiF4(s)+2Br2(l)+3O2(g)

The amount of O2 was calculated from its mass.  Because 1 mol of TiO2 was present in the sample for each mole of O2 isolated.  Therefore amount of TiO2 should be known to calculate its mass and mass percentage in the sample.

The molar mass of O2 is 32.0g/ mol. Then the amount of oxygen can be calculated as follows,

0.143gO2×1molO232.0gO2=0.00446molO2

1 mol of O2 is produced from 1 mol of TiO2, the amount of TiO2 in the sample must also have been 0

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