Chapter 2, Problem 141GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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,

Â Â Â Â Â  xI2â€‰+â€‰yâ€‰â€‰Cl2â€‰â€‰â†’â€‰â€‰2IxCly

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

â€‚Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰Massâ€‰inâ€‰gramsâ€‰Molarâ€‰mass

Therefore,

The number of moles of iodine is,

Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰0.678â€‰â€‰g253.81â€‰g/molâ€‰=â€‰â€‰0.002671â€‰â€‰mol

The number of moles of product IxCly is,

Â Â Â Â 2xâ€‰Ã—â€‰â€‰molesâ€‰â€‰ofâ€‰â€‰I2â€‰â€‰=â€‰â€‰0.005342â€‰/â€‰xâ€‰â€‰mole

Molar mass of IxCly = 1.246â€‰â€‰Ã—â€‰â€‰(0.005342â€‰/â€‰x)â€‰â€‰â€‰=â€‰â€‰â€‰233.22â€‰â€‰/xâ€‰g/mol

Considering the value of x = 1.

Then the molar mass of the compound isâ€‰â€‰233

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