For the reaction2BrF3 (g) → Br₂(g) + 3F₂ (9)AGO 451 kJ andΔΗ°This reaction isfavored under standard conditions at 338 K.The entropy change for the reaction of 1.54 moles of BrF3 (9) at this temperature would be=542 KJ at 338 K and 1 atm.J/K. Consider the reaction:2H₂(g) + O2(g) → 2H₂O(g)Using standard thermodynamic data at 298 K, calculate the free energy change when 2.08 moles of H₂ (g) react at standard conditions.AG°rxnSubstance AG (kJ/mol)H₂O(g) -228.6H₂(g)0.0O₂(g)0.0kJ

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For the reaction 2BrF3 (g) → Br2(g) + 3F₂ (g) AG = 451 kJ and AH° 542 kJ at 338 K and 1 atm. This reaction is favored under standard conditions at 338 K. The entropy change for the reaction of 1.54 moles of BrF3 (9) at this temperature would be J/K.

For the reaction 2BrF3 (g) → Br2(g) + 3F₂ (g) AG = 451 kJ and AH° 542 kJ at 338 K and 1 atm. This reaction is favored under standard conditions at 338 K. The entropy change for the reaction of 1.54 moles of BrF3 (9) at this temperature would be J/K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

For the reaction
2BrF3 (g) → Br₂(g) + 3F₂ (9)
AGO 451 kJ and
ΔΗ°
This reaction is
favored under standard conditions at 338 K.
The entropy change for the reaction of 1.54 moles of BrF3 (9) at this temperature would be
=
542 KJ at 338 K and 1 atm.
J/K.

Consider the reaction:
2H₂(g) + O2(g) → 2H₂O(g)
Using standard thermodynamic data at 298 K, calculate the free energy change when 2.08 moles of H₂ (g) react at standard conditions.
AG°
rxn
Substance AG (kJ/mol)
H₂O(g) -228.6
H₂(g)
0.0
O₂(g)
0.0
kJ

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