Question
Consider the reaction$$2 \mathrm{O}(g) \longrightarrow \mathrm{O}_{2}(g)$$a. Predict the signs of $\Delta H$ and $\Delta S$.b. Would the reaction be more spontaneous at high or low temperatures?
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In this reaction, two oxygen atoms are combining to form an oxygen molecule. This means that the system is going from a more disordered state (individual atoms) to a more ordered state (molecules). Show more…
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Consider the reaction $$\begin{array}{l}{2 \mathrm{O}(g) \longrightarrow \mathrm{O}_{2}(g)} \\ {\text { sof } \Delta H \text { and } \Delta S}\end{array}$$ a. Predict the signs of $\Delta H$ and $\Delta S .$ b. Would the reaction be more spontaneous at high or low temperatures?
Consider the following endothermic decomposition of $\mathrm{AB}_{2}$ molecules: (a) What is the $\operatorname{sign}(+,-, \text { or } 0)$ of $\Delta S^{\circ}$ for the reaction? (b) Is the reaction more likely to be spontaneous at high temperatures or at low temperatures? Explain.
Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each reaction is spontaneous. \begin{equation}\begin{array}{l}{\text { a. } \mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)} \\ {\text { b. } \mathrm{CO}_{2}(s) \longrightarrow \mathrm{CO}_{2}(g)} \\ {\text { c. } \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{H}(g)} \\ {\text { d. } 2 \mathrm\ {NO}_{2}(g) \longrightarrow 2 \mathrm\ {NO}(g)+\mathrm{O}_{2}(g) \text { (endothermic) }}\end{array} \end{equation}
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