   Chapter 5, Problem 36PS

Chapter
Section
Textbook Problem

Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide.CH3OH (ℓ) + CO(g) → CH3CO2H(ℓ)ΔrH°= –134.6 kJ/mol-rxnWhat is the enthalpy change for producing 1.00 L of acetic acid (d = 1.044 g/mL) by this reaction?

Interpretation Introduction

Interpretation:

The enthalpy change for producing a definite volume acetic acid has to be determined.

Concept Introduction:

Standard enthalpy of the reaction,ΔrHo, is the change in enthalpy that happens when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.

Enthalpy of the reaction,ΔrH, is the change in enthalpy that happens when matter is transformed by a given chemical reaction

The change in enthalpy, ΔH in kJ per mole of a given reactant for the reaction can be calculated as:

ΔrH=enthalpy changenumber of moles

ΔrH=ΔHnumber of moles

Explanation

Given,

ΔrHo=-134.6kJ/mol

Mass=1.044g

Determine the no of moles of acetic acid in 1.044g

1.044g(1mol÷60.05 g) =0.01738mol

The change in enthalpy,   in kJ per mole of a given reactant for the reaction can be calculated as:

ΔrH=

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