Molar entropy does not depend on pressure

the enthalpy does not depend on pressure

Cv=Cp-nR

Molar entropy always increases with temprerature

pV is proportional to absolute temperature

ΔT=0

ΔU=w

ΔU=w but only for perfect gas

ΔU=ΔH+Δ(pV) but only for perfect gas

q+w=TΔS

is the the heat effect of reaction of combustion of 1 mole of a compound in air at standard pressure

is equal to TΔcSo+ΔcGo

is defined at standard pressure

doesn’t depend on temperature

is equal to zero

is equal to delta(pV)/T

is equal to -delta(pV)/T

none from above

is equal to (C_v razy delta T)/T

The heat capacity shows a discontinuity

Entropy changes in continous way

thermal expresion coefficient shows a discontinuity

Entropy shows a discontinuity

The transition entropy is delta H=T delta trans S

has a minimum at the critical point

always increases with temperature

can be defined as (dG/dξ)T

at the triple point of a substance is equal for solid, liquid and vapor

doesn’t depend on pressure

is equal to -RTlnx in system (raoult's law)

is 0 for perfect gases

is equal to RTlnx in system (henry's law)

is equal to -Rlnx in system (raoult's law)

is equal to Rlnx in system (henry's law)

depends on the molar fractions of reactants and products in the mixture

does not depend on the total volume of the reaction mixture

does not depend on temperature

depends on the partial pressures in the reaction mixture

has a temperature dependence given by the Van’t Hoff law