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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text: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.

Transcribed Image Text: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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