BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

It has been demonstrated that buckminsterfullerene (C60), another allotrope of carbon (Section 2.3), may be converted into diamond at room temperature and 20,000 atmospheres pressure (about 2 GPa). The standard enthalpy of formation, ΔfH°, for buckminsterfullerene is 2320 kJ/mol at 298.2 K.

  1. a. Calculate ΔrH° for the conversion of C60 to diamond at standard state conditions and 2982 K.
  2. b. Assuming that the standard entropy per mole of carbon in both C60 and diamond is comparable (both about 23 J/K mol), is the conversion of C60 to diamond product-favoredat room temperature?

(a)

Interpretation Introduction

Interpretation:

The ΔrH° for the conversion of C60 to diamond should be be calculated.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and enthalpy by the following expression,

  ΔGo=ΔHo-TΔSo

The sign of ΔGo should be positive for a product-favored reaction. Thus, spontaneous reactions are referred to those that have negative free energy formation.

The standard free enthalpy change is expressed as,

  ΔrH°=fH°(products)fH°(reactants)

Explanation

The ΔrH° for the conversion of C60 to diamond is calculated below.

Given:

Refer to Appendix L for the values of standard enthalpies.

The standard enthalpy value for C60 is 2320 kJ/mol.

The standard enthalpy value for C(diamond) is 1.8 kJ/mol.

The given reaction is,

  C60(s)60 C(diamond)

The standard enthalpy change is,

  ΔrH°=fH°(products)fH°(reactants)=[(60 mol C(diamond)/mol-rxn)ΔfH°

(b)

Interpretation Introduction

Interpretation:

The conversion of C60 to diamond should be identified that it is product favoured at room temperature or not.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and enthalpy by the following expression,

  ΔGo=ΔHo-TΔSo

The sign of ΔGo should be positive for a product-favored reaction. Thus, spontaneous reactions are referred to those that have negative free energy formation.

The standard free enthalpy change is expressed as,

  ΔrH°=fH°(products)fH°(reactants)

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Chapter 18 Solutions

Show all chapter solutions add

Additional Science Solutions

Find more solutions based on key concepts

Show solutions add

Explain Millikans oil-drop experiment.

General Chemistry - Standalone book (MindTap Course List)

Vomiting or diarrhea causes fluid to be pulled from between the cells in every part of the body. causes fluid t...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

What is a joint?

Human Biology (MindTap Course List)

Using the prefix cis- or trans-, name each of the following: a. c. b. d.

Chemistry for Today: General, Organic, and Biochemistry