Chapter 18, Problem 9PS

### Chemistry & Chemical Reactivity

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

Chapter
Section

### Chemistry & Chemical Reactivity

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

# What information is needed to calculate the entropy change that occurs when 1.00 mole of water vapor condenses to liquid water at 100 °C?

Interpretation Introduction

Interpretation: The information needed for calculating the entropy change for the given reaction which occurs when 1mole of water vapor condenses to liquid water at 100oC should be identified.

Concept introduction: The universe consists of two parts, systems and surroundings. The entropy change for the universe is the sum of entropy change for the system and for surroundings.

ΔS(universe)= ΔS(system)+ΔS(surroundings)whereΔS= Entropy change

The ΔS(universe) should be greater than zero for a spontaneous process.

ΔS(system)=ΔrS°=nS°(products)nS°(reactants)whereΔS= Entropy change

ΔS(surroundings)=ΔrHoTwhereΔS= Entropy changeT=TemperatureΔrHo=Enthalpychange

Explanation

The chemical reaction is one mole of water vapour condenses to liquid water at 100oC. The reaction is as follows,

H2O(g)H2O(l)

The entropy change of universe for any reaction is calculated by the following formula

ΔS(universe)= ΔS(system)+ΔS(surroundings)

Thus, ΔS(system) and ΔS(surroundings) both have to be calculated.

The  ΔS(system) can be calculated by the following expression,

ΔS(system)=ΔrS°=nS°(products)nS°(reactants)

The ΔS(surroundings)</

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