Wk.5 Thermodynamics #13

[Jaclyn Padilla]

For a particular reaction, ΔH=−28.4 kJ and ΔS=−87.9 J/K.
Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous?

I will use deltaG=deltaH-TdeltaS to continue on with this question. First I would replace deltaG with 0 since the question is at equilibrium. Then I would arrange the formula arrange so that T=deltaH/deltaS. Next I plug all the values into the question with the appropriate units. Overall my final answer was 323K after converting into kj.

[joselle barnoya 1k]

Hello, I was wondering, for this one, how do we know that the reaction is at equilibrium and that we should replace delta G with 0? Is that why we replace it with 0 or is it because since we are looking at when the reaction is going from nonspontaneous to spontaneous (where spontaneous indicates a negative delta G and nonspontaneous indicates a positive delta G) and that tipping point would be delta G = 0. Since at equilibrium for a reaction G can be positive or negative-- that's what I thought anyways...