   Chapter 2, Problem 141GQ

Chapter
Section
Textbook Problem

Direct reaction of iodine (I2) and chlorine (Cl2) produces an iodine chloride, IxCly, a bright yellow solid. If you completely consume 0.678 g of I2 in a reaction with excess Cl2 and produce 1.246 g of IxCly, what is the empirical formula of the compound? A later experiment showed that the molar mass of IxCly was 467 g/mol. What is the molecular formula of the compound?

Interpretation Introduction

Interpretation: The empirical and molecular formulas for the given IxCly compound should 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

• Equation for number moles from mass and molar mass,

Numberofmoles=MassingramsMolarmass

• Molar mass=Amountofsubstance(mol)×Mass
Explanation

Given,

Direct reaction of iodine and chlorine produces an iodine chloride, IxCly .

The reaction can be represented as,

xI2+yCl22IxCly

Number of moles of elements in the compound can be determined as follows,

Numberofmoles=MassingramsMolarmass

Therefore,

The number of moles of iodine is,

Numberofmoles=0.678g253.81g/mol=0.002671mol

The number of moles of product IxCly is,

2x×molesofI2=0.005342/xmole

Molar mass of IxCly = 1.246×(0.005342/x)=233.22/xg/mol

Considering the value of x = 1.

Then the molar mass of the compound is233

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