Heat-Related Concepts and Quantities

Heat = Energy that is transferred as a consequence of a temperature difference, ΔT.   The possible transfer processes are
              conduction, convection and radiation.

Heat Capacity = The amount of energy,  ΔE, which must be added to a system per unit temperature change, ΔT, in that system,
              i.e., HC =  ΔE / ΔT.

Specific Heat = the heat capacity, HC, per unit mass, Δm, often symbolized by c, i.e., c = HC / Δm = ΔE / (Δm ΔT ).  Note that
              cH2O = 1.00 cal / g°C, cice = 0.50 cal / g°C, cdry air = 0.24 cal / g°C, etc.  The only known substances with specific heats
              greater than water are the gaseous forms of hydrogen and helium and water vapor.

Latent Heat = the amount energy, ΔE, per unit mass, Δm, associated with a particular phase change, i.e., L = ΔE / Δm.

Process Quantity of Substance Temperature (Range) Requires Energy Hence
To Heat 1.0 g of ice from -100°C to 0°C 50 calories cice = 0.50 cal/g°C
To Melt 1.0 g of ice @ 0°C 80 calories Lfusion = 80 cal/g
To Heat 1.0 g of water from 0°C to 100°C 100 calories cH2O = 1.00 cal/g°C
To Evaporate 1.0 g of water @ 100°C 540 calories Lvaporization = 540 cal/g
To Evaporate 1.0 g of water @ 20°C ~600 calories Lv water at 20°C ~ 600 cal/g