   Chapter 5, Problem 63PS

Chapter
Section
Textbook Problem

The enthalpy change for the oxidation of naphthalene, C10Hg, is measured by calorimetry.C10H8(s) + 12 O2(g) → 10 CO2(g) + 4 H2O(ℓ)ΔrH° = –5156.1 kJ/mol-rxnUse this value, along with the standard enthalpies of formation of CO2(g) and H2O(ℓ), to calculate the enthalpy of formation of naphthalene, in kJ/mol.

Interpretation Introduction

Interpretation:

The enthalpy of formation of naphthalene has to be determined.

Concept Introduction:

The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.

Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation

Given,

ΔfH0(CO2)=-393.50kJ/mol

ΔfH0(H2O)=-285.83kJ/mol

ΔfH0(H2O )-241.83kJ/mol

Substitute for the equation,

ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

-5156

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 