Download Thermodynamics Formulas and Sign Conventions and more Study notes Chemistry in PDF only on Docsity! Chapters Five and Nineteen: Thermodynamics āI heard you tellin' Dave to shoot me in the brain with a laser, out behind the dumpster.ā Sign Convention Signs matter. In the case of work and heat, a positive sign (+) means it is ENTERING while an negative sign (-) means it is LEAVING. Units Function Abbreviation Unit State Function? Work w Joules No Heat q Joules No Internal Energy E Joules Yes Enthalpy H Joules Yes Entropy S Joules/Kelvin Yes Gibbs Free Energy G Joules Yes Formulas Most of the work in these two chapters is relatively simple math; the hard part is knowing which formula to use. Formula Important Thingsā¦ When to useā¦ ?E = q + w The 1st law of Thermodynamics Relating internal energy, heat, and work. Always valid. w = -P? V Expansion work; a gas expanding against a pressure P (in Pascals) does work w in Joules. The ? V is the change in volume of the gas; needs to be in m3. Use when a gas it expanding and you need to know something about work. Should be very obvious, as the problem will have to give you both an external pressure and a volume. ?H = qp ONLY AT CONSTANT PRESSURE! ā¦ but lots of things are at constant pressure. Problems at constant pressure always explicitly say so. Tm q atSpecificHe ā = * Temperature has to be in Kelvin. Mass usually needs to be in grams. The word ācalorimeterā really gives things away. ? H0rxn = ? n H 0 products - ?nH 0 reactants DO NOT FORGET MOLAR COEFFICEINTS! This ? H0 isnāt necessarily the same thing as ?H. āstandard molar enthalpy of formationā T q S =ā Temperature has to be in Kelvin. Watch the sign on q; if the system is releasing heat and you want to know the ?S of the surroundings, q needs to be positive. Use when you want to know an entropy change associated with a given heat transfer at a given temperature. T H S trstrs =ā A sort of special case form of the formula above. Watch the sign on H. Phase transitions; melting, freezing, sublimationā¦ ? S0rxn = ? n S 0 products - ?nS 0 reactants DO NOT FORGET MOLAR COEFFICEINTS! This ? S0 is not necessarily the same thing as ?S. āstandard molar entropyā