| Term | Definition |
|---|
| Entropy change | Delta S |
| Enthalpy change | Delta H |
| Standard free energy change | Delta G |
| Gibbs free energy equation | The thermodynamic function defined by the equation G = H – TS, which is used to determine the spontaneity of a reaction. |
| Temperature symbol | T |
| If Delta H is - and Delta S is + then ... | Delta G is - |
| If Delta H is + and Delta S is - then ... | Delta G is + |
| Delta H and S are - the temp. has to be | Low |
| Delta H and S are + the temp. has to be | High |
| From a gas to a liquid Delta S ... | Decreases |
| From 2 moles of gas to one mole of gas Delta S ... | Doesn't change, slightly increases |
| Reaction is spontaneous when Delta G is | Negative |
| When Delta G is + Delta H has to be | Positive |
| When Delta G is - Delta S has to be | Positive |
| ∑H=∑H(?) -∑H(?) | Products-Reactants |
| From a solid to a liquid Delta S ... | Increases |
| Randomness Factor | Nature tens to move spontaneously from an state of lower probability to one of higher probability |
| Units for entropy | J/mol×K |
| Exothermic reactions tend to be... | Spontaneous |
| Equation for Delta G under certian pressures and concentrations | Delta G=Delta G°+RTlnQ |
| R= | .00831 kj/K |
| Free energy changes for multipule reactions equation | Delta G₃=Delta G₁+Delta G₂ |
| Thremodynamic Functions | Delta H, Delta S, Delta G |
| Something that requires no energy to start and can continue by itself with no further imput of energy | Spontaneous processes |
| Second law of thermodynamics | In a spontaneous process, there is a net increase in entropy, taking into account both system and surroundings |
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