Question

1) positive, greater than 0 OR negative, less than 0

FOLLOW-UP PROBLEM 20.7 Determining the Effect of Temperature on AG A reaction is nonspontaneous at room temperature but is spontaneous at 500°C. What can you say about the signs and relative magnitudes of AG, AH, AS, and -TAS? At higher temperatures determine the signs for the following AG is Select HINTS AH is Select Getting Started AS is Select TAS is Select The AH value becomes Select than the -TAS value.

2) positive, greater than 0 OR negative, less than 0

3) positive, greater than 0 OR negative, less than 0

4) positive, greater than 0 OR negative, less than 0

5) smaller, larger, smaller or larger depending on temp.

  

Answer 1

Delta G = Delta H -T Delta S Since the reaction is spontaneous at higher temperature, Delta G is negative. SO, for the reaction to be spontaneous heat energy must be required, as a result of which, the reaction is endothermic in nature and hence, Delta H must be positive. More over, a higher temperature leads to increase in entropy and hence Delta S must be positive. At higher temperature, the reaction is spontaneous when, Delta G = negative Delta H = positive Delta S = positive Since, Delta G = Delta H -T Delta S Delta G will be negative only when, Delta H is greater than T Delta S

Since the reaction is spontaneous at higher temperature, $\Delta$ G is negative. SO, for the reaction to be spontaneous heat energy must be reuired, as a result of which, the reaction is endothermic in nature and hence, $\Delta$ H must be positive. More over, a higher temperature leads to increase in entropy and hence $\Delta$ S must be positive.

At higher temperature, the reaction is spontneous when,

$\Delta$ G = negative    $\Delta$ H= positive $\Delta$ S = positive

Since,

Delta G = Delta H -T Delta S Since the reaction is spontaneous at higher temperature, Delta G is negative. SO, for the reaction to be spontaneous heat energy must be required, as a result of which, the reaction is endothermic in nature and hence, Delta H must be positive. More over, a higher temperature leads to increase in entropy and hence Delta S must be positive. At higher temperature, the reaction is spontaneous when, Delta G = negative Delta H = positive Delta S = positive Since, Delta G = Delta H -T Delta S Delta G will be negative only when, Delta H is greater than T Delta S

$\Delta$ G will be negative only when, $\Delta$ H is greater than T $\Delta$ S