   Chapter 4, Problem 89GQ

Chapter
Section
Textbook Problem

Silicon and hydrogen form a series of compounds with the general formula SixHy. To find the formula of one of them, a 6.22-g sample of the compound is burned in oxygen. All of the Si is converted to 11.64 g of SiO2, and all of the H is converted to 6.980 g of H2O. What is the empirical formula of the silicon compound?

Interpretation Introduction

Interpretation:

The empirical formula of silicon compound in the given sample has to be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Equation for finding Molecular formula from the empirical formula,

MolarmassEmpiricalformula mass × Empirical formula

• 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).
Explanation

Herein 6.22g of silicon compound burns in oxygen then give 11.64g of SiO2 and 6.980g of H2O

From the given masses the amount of SiO2andH2O can be calculated.

Thus, amount of SiO2andH2O are,

11.64gSiO2×1molSiO260.08gSiO2=0.1937molSiO26.980gH2O×1molH2O18.015gH2O=0.3874molH2O

For every mole of SiO2 isolated, 1 mol of Si must have been present in the silicon compound.

So,

0.1937molSiO2×1molSiinmenthol1molSiO2=0

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