PLEASE HELP I DO NOT UNDERSTAND THIS AT ALL :(
Describe in detail what you know about the enthalpy, entropy, and free energy changes when a sample of gas condenses to a liquid. How does temperature affect these changes?
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Do not post the same question more than once. It's annoying. Use \[\Delta G = \Delta H - T \Delta S\]
Since we're going from a high temp to a low temp(gas to liquid) H will be negative meaning it gives off energy. We are also going from less ordered to more ordered. (gas is random and crazy to a more ordered liquid) Therefore entropy is negative since we know that entropy is positive when we go from a liquid to a gas it's just the opposite. We also know that when delta G is negative the reaction is spontaneous.So how do we find when delta G is negative. That depends on temp. \[\Delta G = (-\Delta H) - (T(-\Delta S))\]When T is large then delta G is positive and the reaction is not spontaneous.
When T is small delta G is negative and the reaction is spontaneous. This means at high temperatures water will not condense but at lower temps it will.