Thermodynamics Flashcards
First Law of Thermodynamics
Heat and energy are not created nor destroyed
Second Law of Thermodynamics
If the forward reaction is spontaneous, then the reverse reaction cannot also be spontaneous
Standard Conditions
Pressure at 1 atm
Solid and Liquids in pure state
298 K or 25 C
Energy of Formation = 0
Enthalpy (ΔH)
Change in Heat over the reaction ΔH (-) -> Reaction is exothermic ΔH (+) -> Reaction in endothermic ΔH= H(products-H reaction ΔH= bonds broken- bonds formed
Hess Law
Apply whatever has been done in the reaction to the ΔH
Heat Capacity
C(p)= ΔH/ΔT
Specific Heat
The amount of heat required to raise 1 gram of substance 1 degree celcius
q= mcΔT
Entropy( ΔS)
- Measures the randomness or disorder of the system,
Solid> Aqueous >Liquid>Gas— Higher Entropy
More moles—Higher Entropy
Gibbs Free Energy
ΔG (-) > Reaction is spontaneous
ΔG(+) > Reaction is not spontaneous
Gibbs Free Energy Calculation
ΔG=ΔH-TΔS
Standard Free Energy Change and Normal
ΔG= ΔGs +RTln(Q)=ΔGs+2.303RTlog(Q)
Standard Free Energy and the Equilibrium Constant
ΔG=-RTln(K)= -2.303RTlog(K)