Calculate Δ r S ° for the following reaction at 25 ° C. 2 H 2 (g) + O 2 (g) → 2 H 2 O(ℓ) (a) − 326.6 J/K · mol-rxn (b) − 139.9 J/K · mol-rxn (c) 139.9 J/K · mol-rxn (d) 326.6 J/K · mol-rxn

Chemistry & Chemical Reactivity

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

Chapter
Section

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18.4, Problem 3RC
Textbook Problem
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Calculate ΔrS° for the following reaction at 25 ° C.2 H2(g) + O2(g) → 2 H2O(ℓ) (a) − 326.6 J/K · mol-rxn (b) − 139.9 J/K · mol-rxn (c) 139.9 J/K · mol-rxn (d) 326.6 J/K · mol-rxn

Interpretation Introduction

Interpretation: the value of ΔrS for the given reaction is to be identified from the given options.

Concept introduction:

In Spontaneous process, energy transfer from higher concentration to lower, or the energy is dispersed.

Entropy (S) is the quantity to measure the dispersal of energy in the spontaneous processes.

ΔrS is the change in entropy at standard condition and it is calculated by sum of the product of stoichiometric coefficients and molar entropies of products minus sum of the product of stoichiometric coefficients and molar entropies of reactants. That is,

ΔrS=nS(products)nS(reactants)

Explanation of Solution

For the reaction,

Coefficient of product H2O is 2 and its molar entropy is 69.9J/Kmol .

Coefficients of reactants H2 and O2 are 2 and 1 respectively and their molar entropy are 130.7J/Kmol and 205.07J/Kmol respectively.

The equation for finding ΔrS is,

ΔrS=nS(products)nS(reactants)

Therefore,

The change in entropy is,

ΔrS=2×69.9J/Kmol(2×130

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