Question

For the reaction \[ \begin{array}{l} 2 \mathrm{BrF}_{3}(\mathrm{~g}) \longrightarrow \mathrm{Br}_{2}(\mathrm{~g})+3 \mathrm{~F}_{2}(\mathrm{~g}) \\ \Delta \mathrm{H}^{\circ}=542 \mathrm{~kJ} \text { and } \Delta \mathrm{S}^{\circ}=269 \mathrm{~J} / \mathrm{K} \end{array} \] The equilibrium constant, \( K \), would be greater than 1 at temperatures \( \square \) Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that \( \Delta \mathrm{H}^{\circ} \) and \( \Delta \mathrm{S}^{\circ} \) are constant.

          For the reaction
\[
\begin{array}{l}
2 \mathrm{BrF}_{3}(\mathrm{~g}) \longrightarrow \mathrm{Br}_{2}(\mathrm{~g})+3 \mathrm{~F}_{2}(\mathrm{~g}) \\
\Delta \mathrm{H}^{\circ}=542 \mathrm{~kJ} \text { and } \Delta \mathrm{S}^{\circ}=269 \mathrm{~J} / \mathrm{K}
\end{array}
\]

The equilibrium constant, \( K \), would be greater than 1 at temperatures \( \square \) Kelvin.

Select above or below in the first box and enter the temperature in the second box. Assume that \( \Delta \mathrm{H}^{\circ} \) and \( \Delta \mathrm{S}^{\circ} \) are constant.

For the reaction

2 BrF3( g) ⟶Br2( g)+3 F2( g)
ΔH^∘=542 kJ and ΔS^∘=269 J / K

The equilibrium constant, K, would be greater than 1 at temperatures □ Kelvin.

Select above or below in the first box and enter the temperature in the second box. Assume that ΔH^∘ and ΔS^∘ are constant.

Added by Andrew C.

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