   Chapter 5, Problem 60PS

Chapter
Section
Textbook Problem

The Romans used calcium oxide, CaO, to produce a strong mortar to build stone structures. Calcium oxide was mixed with water to give Ca(OH)2, which reacted slowly with CO2 in the air to give CaCO3.Ca(OH)2(s) + CO2(g) → CaCO3(s) + H2O(g)(a) Calculate the standard enthalpy change for this reaction.(b) How much energy is evolved or absorbed as heat if 1.00 kg of Ca(OH)2 reacts with a stoichiometric amount of CO2?

(a)

Interpretation Introduction

Interpretation:

The standard enthalpy of reaction 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(Ca(OH)2)= -987kJ/mol

ΔfH0(CaCO3)=-1207kJ/mol

ΔfH0(H2O)=-241.83kJ/mol

ΔfH0(CaO) =-636kJ/mol

ΔrH0=[(1mol)(-1207kJ/mol)+(1mol)(-241

(b)

Interpretation Introduction

Interpretation:

The heat evolved or absorbed 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)

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

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