Chemical Thermodynamics

A system is the part

A system is the part of universe under study, while surroundings include everything else. Systems can be open (exchange both matter and energy), close

State functions (like P

State functions (like P, V, T, U, H, S, G) depend only on the current state, not on how that state was reached. Path functions (like Q and W) depend o

States that energy cannot be created

States that energy cannot be created or destroyed, only converted. Mathematically: ΔU = Q + W, where ΔU is change in internal energy, Q is heat added

Defined as H = U +

Defined as H = U + PV. For reactions at constant pressure, ΔH = Qp (heat absorbed at constant pressure). Related to internal energy by ΔH = ΔU + ΔngRT

A measure of molecular disorder

A measure of molecular disorder or randomness in a system. ΔS = Qrev/T for reversible processes. Entropy increases from solid → liquid → gas phases an