Question

For the reaction \[ \begin{array}{l} 2 \mathrm{NH}_{3}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\ \Delta \mathrm{H}^{\circ}=-683 \mathrm{~kJ} \text { and } \Delta \mathrm{S}^{\circ}=-366 \mathrm{~J} / \mathrm{K} \end{array} \] The equilibrium constant, \( \mathrm{K} \), 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
\[
\begin{array}{l}
2 \mathrm{NH}_{3}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\
\Delta \mathrm{H}^{\circ}=-683 \mathrm{~kJ} \text { and } \Delta \mathrm{S}^{\circ}=-366 \mathrm{~J} / \mathrm{K}
\end{array}
\]

The equilibrium constant, \( \mathrm{K} \), 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 NH3( g)+2 O2( g) ⟶N2O(g)+3 H2O(l)
ΔH^∘=-683 kJ and ΔS^∘=-366 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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