Question

question 6
at 298 k, what is the effect of increasing the temperature on the standard free - energy change for a reaction with negative δs and a positive δh?
increases δg
decreases δg
no effect on δg
δg becomes zero
question 7
which of the following is not a way to calculate δg of a reaction?
use the equation δg = δh - tδs
(sum of δg°s of products) - (sum of δg°s reactants)
add the δg°s of several known reactions, similar to hesss law
determine the value using coulombs law

Explanation:

Step1: Recall the Gibbs - free energy equation

The equation is $\Delta G=\Delta H - T\Delta S$. Given $\Delta H> 0$ and $\Delta S<0$.

Step2: Analyze the effect of temperature increase

As $T$ increases, the term $-T\Delta S$ (since $\Delta S < 0$, $-T\Delta S>0$) becomes more positive. And $\Delta H>0$. So $\Delta G=\Delta H - T\Delta S$ increases as $T$ increases.

Answer:

Increases $\Delta G$