For the reaction\[ 2\text{BrF}_3(g) \rightarrow \text{Br}_2(g) + 3\text{F}_2(g) \]\[\Delta G^\circ = 471\ \text{kJ} \quad \text{and} \quad \Delta H^\circ = 542\ \text{kJ} \quad \text{at 264 K and 1 atm}.\]This reaction is \(\blacksquare\) favored under standard conditions at 264 K.The entropy change for the reaction of 2.39 moles of \(\text{BrF}_3(g)\) at this temperature would be \(\blacksquare\) J/K.

Recall the given reaction, Number of moles of

For the reaction 2BrF3 (g) → Br₂(g) + 3F₂ (g) AG = 471 kJ and AH° = 542 kJ at 264 K and 1 atm. This reaction is reactant favored under standard conditions at 264 K. The entropy change for the reaction of 2.39 moles of BrF3 (9) at this temperature would be J/K.

For the reaction 2BrF3 (g) → Br₂(g) + 3F₂ (g) AG = 471 kJ and AH° = 542 kJ at 264 K and 1 atm. This reaction is reactant favored under standard conditions at 264 K. The entropy change for the reaction of 2.39 moles of BrF3 (9) at this temperature would be J/K.

Chemistry

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Chapter1: Chemical Foundations

Section: Chapter Questions

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For the reaction

\[ 2\text{BrF}_3(g) \rightarrow \text{Br}_2(g) + 3\text{F}_2(g) \]

\[
\Delta G^\circ = 471\ \text{kJ} \quad \text{and} \quad \Delta H^\circ = 542\ \text{kJ} \quad \text{at 264 K and 1 atm}.
\]

This reaction is \(\blacksquare\) favored under standard conditions at 264 K.

The entropy change for the reaction of 2.39 moles of \(\text{BrF}_3(g)\) at this temperature would be \(\blacksquare\) J/K.

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