   # Given the enthalpy of formation data below, calculate Δ soln H ° for LiOH. ∆ f H ° [LiOH(s)] = − 484.93 kJ/mol ∆ f H ° [LiOH(aq)] = − 508.48 kJ/mol (a) +23.55 kJ/mol (b) +993.41 kJ/mol (c) −23.55 kJ/mol (d) −993.41 kJ/mol ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13.2, Problem 1RC
Textbook Problem
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## Given the enthalpy of formation data below, calculate Δ solnH° for LiOH. ∆fH° [LiOH(s)] = − 484.93 kJ/mol ∆fH° [LiOH(aq)] = − 508.48 kJ/mol (a) +23.55 kJ/mol (b) +993.41 kJ/mol (c)    −23.55 kJ/mol(d)    −993.41 kJ/mol

Interpretation Introduction

Interpretation: The enthalpy of solution of LiOH is to be determined from the given option.

Concept introduction:

Enthalpy of solution: In the process, the change in enthalpy while dissolving the solute in the solvent.

The enthalpy of solution is calculated by the formula

ΔsolnH0=Σ(nΔfH0(product))Σ(nΔfH0(reactant))

### Explanation of Solution

Reason for correct option

Given,

Enthalpy of formation of LiOHin the solid state =484.93 kJ/molEnthalpy of formation of LiOHin the solution    =508.48 kJ/mol

The enthalpy of solution is calculated by the formula

ΔsolnH0=Σ(nΔfH0(product))Σ(nΔfH0(reactant))

The enthalpy of solution of LiOH is,

ΔsolnH0=ΔfHo[LiOH(aq)]-

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