𝚫Hfus, endothermic, negative value

𝚫Hvap, exothermic, positive value

𝚫Hfus, endothermic, positive value

𝚫Hvap, endothermic, positive value

q = mc𝚫T

q = nCm𝚫T

𝚫Hsub = 𝚫Hfus + 𝚫Hvap

𝚫Gº = 𝚫Hº - T𝚫Sº

It takes a large amount of energy to increase the temperature

It takes less time to increase the temperature

Retains heat longer

ΔH =
ΣBE_{(bonds broken)} - ΣBE_{(bonds formed)}

ΔHºrxn=
∑ΔHºf(products)−
∑ΔHºf(Reactants)

q = mcΔT

All energy in chemical and physical is conserved

An equilibrium system will shift to reduce pressure

The enthalpy change is equal to the sum of the enthalpy changes for each step

The distribution of kinetics energies increases as temperature increases