Consider the reaction: 2 KClO3 (s) = 2 KCl (s) + 3 O2 (g). Based on the following data of standard molar enthalpy of formation of ΔHf° and standard molar entropy ᔆ?°, determine the standard Gibbs free energy change of the above reaction ΔGᵣₓₙ° at 87.0 °C (in kJ with 3 significant figures). KClO3 (s) KCl (s) O2(g) ΔHf° (kJ/mol) -391.204 -435.89 0 Δᔆ?° (J/K-mol) 142.97 239.49 205.03 Note that ΔHf° and Δᔆ?° are temperature independent.
Consider the reaction: 2 KClO3 (s) = 2 KCl (s) + 3 O2 (g). Based on the following data of standard molar enthalpy of formation of ΔHf° and standard molar entropy ᔆ?°, determine the standard Gibbs free energy change of the above reaction ΔGᵣₓₙ° at 87.0 °C (in kJ with 3 significant figures). KClO3 (s) KCl (s) O2(g) ΔHf° (kJ/mol) -391.204 -435.89 0 Δᔆ?° (J/K-mol) 142.97 239.49 205.03 Note that ΔHf° and Δᔆ?° are temperature independent.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Consider the reaction: 2 KClO3 (s) = 2 KCl (s) + 3 O2 (g).
Based on the following data of standard molar enthalpy of formation of ΔHf° and standard molar entropy ᔆ?°, determine the standard Gibbs free energy change of the above reaction ΔGᵣₓₙ° at 87.0 °C (in kJ with 3 significant figures).
KClO3 (s) KCl (s) O2(g)
ΔHf° (kJ/mol) -391.204 -435.89 0
Δᔆ?° (J/K-mol) 142.97 239.49 205.03
Note that ΔHf° and Δᔆ?° are temperature independent.
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