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Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I ) s u l f a t e ( a q ) c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I I ) s u l f a t e ( a q ) You place 87.7 mL of a 0.500- M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 132CP
Textbook Problem
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Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations.

c o p p e r ( I I )   s u l f a t e ( a q )   +   i r o n ( s ) c o p p e r ( s )   +   i r o n ( I I )   s u l f a t e ( a q ) c o p p e r ( I I )   s u l f a t e ( a q )   +   i r o n ( s ) c o p p e r ( s )   +   i r o n ( I I I )   s u l f a t e ( a q )

You place 87.7 mL of a 0.500-M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.

Interpretation Introduction

Interpretation: The reaction that produces a better yield of copper has to be identified.

Concept Introduction: The mass of the compound is calculated by taking the products of molar mass of the compound to the given mass. The mass of compound can be given by,

Massofcompound(ingrams)=Molarmass(ing)×Givenmass(ing)

Explanation of Solution

Explanation

Record the given data

Volume of Copper sulphate = 87.7mL

Molarity of Copper sulphate = 0.500M

Amount of Iron added          = 2.00g

Amount of Copper isolated = 2.27g

The volume and molarity of Copper sulphate along with amount of Iron and amount of Copper are recorded as shown above.

To calculate the moles of Cu and Fe

Molar mass of Fe = 55.85g

MolesofCu=87.7mL×1L1000mL×0.500molL=0.0439molMolesofFe=2.001molFe55.85g=0.0358mol

The moles of copper are calculated by plugging in the values of volume and molarity of Copper sulphate and moles of Iron is calculated by plugging in the values of grams of Iron added to the molar mass of Iron. The moles of Copper and Iron are found to be 0.0439mol and 0.0358mol respectively.

To predict which of the two reactions gives better yield

Moles of Copper = 0.0439mol

Moles of Iron      = 0.0358mol

Molar mass of Copper = 63.55g

The two possible reactions are,

ReactionI,CuSO4(aq)+Fe(s)Cu(s)+FeSO4(aq)ReactionII,2CuSO4(aq)+2Fe(s)3Cu(s)+Fe2(SO4)3(aq)

For reaction I, if iron is limiting,

AmountofCopperisolated=0

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Chapter 6 Solutions

Chemistry: An Atoms First Approach
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