If ∆S is negative, then the negative signs (from the subtraction and the sign of ∆S) will cancel out, and so as T∆S gets bigger, ∆G will get more positive. T is always positive, so if ∆S is positive then a bigger T∆S will make ∆G more negative (since we subtract T∆S). As T increases, the T∆S component gets bigger. ∆H is still positive and ∆S is still whatever sign you figured out above. The energy of a system can change due to work and other forms of energy transfer such as heat. Since ∆H and ∆S don't change significantly with temperature (given in the question), we can assume that they keep the same signs and values: i.e. Google Classroom The meaning of work in thermodynamics, and how to calculate work done by the compression or expansion of a gas Key Points: Work is the energy required to move something against a force. If ∆G is negative (from the question), is the reaction spontaneous or non-spontaneous?Ģ) Let's use ∆G = ∆H - T∆S again. A tool perform calculations on the concepts and applications for Thermochemistry calculations. From these values, we can know for certain whether ∆S is positive or negative (hint: remember that we are subtracting ∆G!).ġ) Knowing the sign of ∆G is enough to say whether the reaction is spontaneous or not under these conditions. Temperature is always positive (in Kelvin). We know (from the question) that ∆G is negative and that ∆H is positive. This looks like a homework question, so I'll give you some hints to get you on the riht path rather than answering directly.ģ) We know that ∆G = ∆H - T∆S.
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