Thermodynamics Formulas - Chemistry · PDF fileThermodynamics Formulas Name Formula 1st Law...
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Thermodynamics Formulas Name Formula 1 st Law of Thermodynamics Δ E universe =Δ E system +Δ E surroundings Energy cannot be created nor destroyed – only change forms. 2 nd Law of Thermodynamics Δ S universe =Δ S sys +Δ S surr ≥ 0 Entropy of the universe is always increasing. 3 rd Law of Thermodynamics S = K B lnW = K B ln (1)= 0 S of a pure crystal at 0K is 0 J/mol·K Enthalpy Δ H = q Enthalpy, ΔH, is the measure of heat energy in a system at constant pressure. Standard Enthalpy Δ H° = ∑ Δ H° f ,products + ∑ Δ H° f , reactants Enthalpy change when one mole of a substance is made from its elements in standard conditions. (Enthalpy Change of Formation) Entropy Δ S = q reversible T Entropy, ΔS, is the measure of disorder in a system. A higher entropy = A greater amount of disorder. Solids < Liquids < Gases. Δ S surroundings =− Δ H system T Standard Entropy Δ S° = ∑ Δ S° products + ∑ Δ S° reactants (Standard Molar Entropies) Gibb's Free Energy Δ G = ∑ Δ G products + ∑ Δ G reactants Used to to predict whether a process will occur spontaneously at a constant temperature and pressure. Δ G =Δ H − T Δ S Δ G =Δ G° + RT ⋅ ln( Q) Q = Reaction Quotient R = 8.3145 J/mol·K Standard Free Energy Δ G° = ∑ Δ G° f ,products + ∑ Δ G° f , reactants Specific Heat Capacity, c q = mc Δ T The amount of heat energy needed to raise the temperature of 1 gram of a substance by 1℃. Used in "coffee-cup" calorimetry. m = mass in grams. (Specific Heat Capacities) Heat Capacity, C q = C Δ T The amount of energy required to raise the temperature of a substance by 1℃. Used in "bomb" calorimetry.
Transcript of Thermodynamics Formulas - Chemistry · PDF fileThermodynamics Formulas Name Formula 1st Law...
Thermodynamics Formulas
Name Formula
1st Law ofThermodynamics
ΔEuniverse = ΔEsystem + ΔEsurroundings Energy cannot be created nordestroyed – only change forms.
2nd Law ofThermodynamics
ΔSuniverse = ΔSsys + ΔSsurr ≥ 0 Entropy of the universe is alwaysincreasing.
3rd Law ofThermodynamics
S= KB lnW =KBln(1) = 0 S of a pure crystal at 0K is 0 J/mol·K
Enthalpy ΔH= q Enthalpy, ΔH, is the measure ofheat energy in a system at constant
pressure.
Standard Enthalpy ΔH°=∑ ΔH° f ,products +∑ ΔH° f , reactants Enthalpy change when one mole ofa substance is made from its
elements in standard conditions.(Enthalpy Change of Formation)
EntropyΔS=
qreversibleT
Entropy, ΔS, is the measure ofdisorder in a system.
A higher entropy = A greateramount of disorder.
Solids < Liquids < Gases.
ΔSsurroundings =−ΔHsystemT
Standard Entropy ΔS°= ∑ΔS°products+∑ ΔS°reactants (Standard Molar Entropies)
Gibb's Free Energy ΔG =∑ΔGproducts +∑ ΔGreactants Used to to predict whether aprocess will occur spontaneously
at a constant temperature andpressure.
ΔG= ΔH − TΔS
ΔG= ΔG° + RT⋅ln(Q) Q = Reaction QuotientR = 8.3145 J/mol·K
Standard Free Energy ΔG°=∑ ΔG° f ,products +∑ ΔG°f , reactants
Specific HeatCapacity,
c
q =mcΔT The amount of heat energy neededto raise the temperature of 1 gram
of a substance by 1℃.Used in "coffee-cup" calorimetry.
m = mass in grams.(Specific Heat Capacities)
Heat Capacity, C
q =CΔT The amount of energy required toraise the temperature of a
substance by 1℃.Used in "bomb" calorimetry.
