17. For Relationship of \( \Delta G, \Delta H \), and \( \Delta S, \Delta G=\Delta H \) - T \( \Delta S \), which one iv(are) righr? A. if \( \mathrm{AH} \propto 0, \mathrm{AS}>0, \mathrm{~A} \) is always negative. Reaction proceeds spoetaneously at all Temperatures. B, if \( \mathrm{AH}<0, \mathrm{\Delta S}>0 \), Reaction proceeds spontaneously at low temperatures. At high Temperatures, the reverse reaction becomes spontancous C. None of them. D. All of \( \mathrm{A} \) and \( \mathrm{B} \).
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If ΔH is approximately 0 and ΔS is greater than 0, then ΔG will be negative because it is equal to ΔH - TΔS. Since ΔH is approximately 0, ΔG is approximately equal to -TΔS. Since T (temperature) is always positive and ΔS is given as positive, ΔG will be negative. Show more…
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From the values of $\Delta H$ and $\Delta S$, predict which of the following reactions would be spontaneous at $25^{\circ} \mathrm{C}$ : reaction $\mathrm{A}$ : $\Delta H=10.5 \mathrm{kJ} / \mathrm{mol}, \Delta S=30 \mathrm{J} / \mathrm{K} \cdot \mathrm{mol} ;$ reaction $\mathrm{B}: \Delta H=$ $1.8 \mathrm{kJ} / \mathrm{mol}, \Delta S=-113 \mathrm{J} / \mathrm{K} \cdot$ mol. If either of the reactions is nonspontaneous at $25^{\circ} \mathrm{C},$ at what temperature might it become spontaneous?
Replace each question mark with the correct information: $$ \begin{array}{lcccl} & \Delta S_{\text {rxn }} & \Delta H_{\text {rxn }} & \Delta G_{\text {rxn }} & \text { Comment } \\ \hline \text { (a) } & + & - & - & ? \\ \text { (b) } & ? & 0 & - & \text { Spontaneous } \\ \text { (c) } & - & + & ? & \text { Not spontaneous } \\ \text { (d) } & 0 & ? & - & \text { Spontaneous } \\ \text { (e) } & ? & 0 & + & ? \\ \text { (f) } & + & + & ? & T \Delta S>\Delta H \end{array} $$
From the values of $\Delta H$ and $\Delta S$, predict which of the following reactions would be spontaneous at $25^{\circ} \mathrm{C}$ : Reaction $\mathrm{A}: \Delta H=10.5 \mathrm{kJ} / \mathrm{mol}, \Delta S=30 \mathrm{J} / \mathrm{K} \cdot \mathrm{mol};$ reaction $\mathrm{B}: \Delta H=1.8 \mathrm{kJ} / \mathrm{mol}, \Delta S=-113 \mathrm{J} / \mathrm{K} \cdot \mathrm{mol}.$ If either of the reactions is nonspontaneous at $25^{\circ} \mathrm{C},$ at what temperature might it become spontaneous?
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