Use the given standard entropy values to calculate the standard entropy change to convert hydrogen chloride to chlorine in the given reaction: 4HCl ₍g₎ + O2₍g₎ → 2Cl₂₍g₎ + 2H₂O₍g₎ S°(J/K•mol): HCl ₍g₎ = 186.8 O2₍g₎ = 205 Cl2₍g₎ = 223 H2O₍g₎ = 188.7
Use the given standard entropy values to calculate the standard entropy change to convert hydrogen chloride to chlorine in the given reaction: 4HCl ₍g₎ + O2₍g₎ → 2Cl₂₍g₎ + 2H₂O₍g₎ S°(J/K•mol): HCl ₍g₎ = 186.8 O2₍g₎ = 205 Cl2₍g₎ = 223 H2O₍g₎ = 188.7
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
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SOLVE THE FOLLOWING PROBLEMS. Write down your answers CLEARLY. Thank you!
Lesson Topic: THERMODYNAMICS (Spontaneous reactions and Gibbs free energy)
1. Use the given standard entropy values to calculate the standard entropy change to convert
hydrogen chloride to chlorine in the given reaction:
4HCl
₍g₎ + O2₍g₎ → 2Cl₂₍g₎ + 2H₂O₍g₎
S°(J/K•mol): HCl
₍g₎ = 186.8
O2₍g₎ = 205
Cl2₍g₎ = 223
H2O₍g₎ = 188.7
2. Predict whether the following reaction leads to an increase or a decrease in entropy. Explain Why.
Ag+₍aq₎ + Cl-₍aq₎ → AgCl₍s₎
3. Calculate ∆G° for the combustion of ethane
2C₂H₆₍g₎ + 7O₂₍g₎ → 4CO₂₍g₎ + 6H₂O₍ₗ₎
With the following ∆G°f:
C₂H₆(g = -32.86 kJ/mol
CO₂(g) = -394.4 kJ/mol
H₂O(l) = -237.2 kJ/mol
O₂(g) = 0
4. From the following ∆H and ∆S values, predict whether the reaction would be spontaneous. If not, at what temperature might the reaction become spontaneous?
∆H = -126 kJ ∆S = 84 J/K
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