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ΔSº and ΔHº question
Posted: Wed Feb 20, 2019 5:50 pm
by Chloe Thorpe 1J
Why can we assume that ΔSº and ΔHº are constant in the Van't Hoff Equation?
Re: ΔSº and ΔHº question
Posted: Wed Feb 20, 2019 5:51 pm
by Mindy Kim 4C
Generally, the change in enthalpy or entropy do not change with temperature. The standard entropies and enthalpies may be different for the compounds, but the change in enthalpy or entropy for the reaction does not vary significantly with change in temperature.
Re: ΔSº and ΔHº question
Posted: Wed Feb 20, 2019 6:22 pm
by Tuong Nguyen 2I
Yes only free energy can be greatly influenced by a change in temperature.
Re: ΔSº and ΔHº question
Posted: Thu Feb 21, 2019 1:36 am
by LeannaPhan14BDis1D
Free energy is the one that changes and is influenced by temperature
Re: ΔSº and ΔHº question
Posted: Thu Feb 21, 2019 1:46 am
by Celio_G_Dis2C
T will mostly affect free energy only. One might think that it also changes enthalpy because the addition of heat will change the forward/irreversible reactions of an equation but the change is minimal
Re: ΔSº and ΔHº question
Posted: Thu Feb 21, 2019 11:38 am
by Hedi Zappacosta 1E
The change in delta S and delta H is negligible with a change in temperature so we assume they are constant.