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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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Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 16, Problem 93AE
Textbook Problem
885 views

Consider the reaction

Fe 2 O 3 ( s ) + 3 H 2 ( g ) 2 Fe ( s ) + 3 H 2 O ( g )

Assuming ∆H° and ∆S° do not depend on temperature, calculate the temperature where K = 1.00 for this reaction.

Interpretation Introduction

Interpretation: The reaction between Fe2O3(s) and H2(g) is given. The temperature at which the value of K is 1.00 is to be calculated.

Concept introduction: The expression for free energy change is,

ΔG°=RTln(K)

And,

ΔG°=ΔH°TΔS°

Hence,

ΔH°TΔS°=RTln(K)

Explanation of Solution

The stated reaction is,

Fe2O3(s)+3H2(g)2Fe(s)+3H2O

Refer Appendix 4 .

The value of ΔH°(kJ) for the given reactant and product is,

Molecules ΔH°(kJ)
Fe2O3(s) 826
Fe(s) 0
H2(g) 0
H2O(g) 242

The formula of ΔH° is,

ΔH°=npΔH°(product)nfΔH°(reactant)

Where,

  • ΔH° is the standard enthalpy of reaction.
  • np is the number of moles of each product.
  • nr is the number of moles each reactant.
  • ΔH°(product) is the standard enthalpy of product at a pressure of 1atm .
  • ΔH°(reactant) is the standard enthalpy of reactant at a pressure of 1atm .

Substitute all values from the table in the above equation.

ΔH°=npΔH°(product)nfΔH°(reactant)=[2(0)+3(242){(826)+3(0)}]kJ=100kJ_

Refer to Appendix 4 .

The value of ΔS°(J/K) for the given reactant and product is,

Molecules ΔS°(J/K)
Fe2O3(s) 90
Fe(s) 131
H2(g) 27
H2O(g) 189

The formula of ΔS° is,

ΔS°=npΔS°(product)nfΔS°(reactant)

Where,

  • ΔS° is the standard enthalpy of reaction.
  • np is the number of moles of each product

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Chapter 16 Solutions

Chemistry: An Atoms First Approach
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Ch. 16 - For the process A(l) A(g), which direction is...Ch. 16 - For a liquid, which would you expect to be larger,...Ch. 16 - Gas A2 reacts with gas B2 to form gas AB at a...Ch. 16 - What types of experiments can be carried out to...Ch. 16 - A friend tells you, Free energy G and pressure P...Ch. 16 - You remember that G is related to RT ln(K) but...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Is Ssurr favorable or unfavorable for exothermic...Ch. 16 - At 1 atm, liquid water is heated above 100C. 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K:...Ch. 16 - Consider the following reaction at 298 K:...Ch. 16 - Consider the relationship In(K)=HRT+SR The...Ch. 16 - The equilibrium constant K for the reaction...Ch. 16 - Using Appendix 4 and the following data, determine...Ch. 16 - Some water is placed in a coffee-cup calorimeter....Ch. 16 - Consider the following system at equilibrium at...Ch. 16 - Calculate the entropy change for the vaporization...Ch. 16 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 16 - Consider the following reaction:...Ch. 16 - Using the following data, calculate the value of...Ch. 16 - Many biochemical reactions that occur in cells...Ch. 16 - Carbon monoxide is toxic because it bonds much...Ch. 16 - In the text, the equation G=G+RTIn(Q) was derived...Ch. 16 - Consider the reactions...Ch. 16 - Use the equation in Exercise 79 to determine H and...Ch. 16 - Consider the reaction...Ch. 16 - Consider the following diagram of free energy (G)...Ch. 16 - Which of the following reactions (or processes)...Ch. 16 - For rubidium Hvapo=69.0KJ/mol at 686C, its boiling...Ch. 16 - Given the thermodynamic data below, calculate S...Ch. 16 - Consider the reaction: H2S(g)+SO2(g)3S(g)+2H2O(l)...Ch. 16 - The following reaction occurs in pure water:...Ch. 16 - Consider the dissociation of a weak acid HA (Ka =...Ch. 16 - Consider the reaction: PCl3(g)+Cl2(g)PCl5(g) At...Ch. 16 - The equilibrium constant for a certain reaction...Ch. 16 - For the following reactions at constant pressure,...Ch. 16 - The standard enthalpy of formation of H2O(l) at...Ch. 16 - Consider two perfectly insulated vessels. 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