Thermal Energy & Heat. What is Temperature? Temperature  measure

Temperature Conversions o C to o F: o F = 9/5( o C) + 32 o F to o C: o C = 5/9( o F – 32) o C to K: K = o C K to o C: o C = K – 273
What is Temperature Temperature  measure of the average KE of all the particles within an object
o F = 9/5( o C) + 32 o F = 9/5(37 o C) + 32 = = 98.6 o F.
Going from Fahrenheit to Celsius Convert 68 o F to o C o C = 5/9( o F – 32) o C = 5/9(68 – 32) = 5/9(36) = 20 o C
Going from Celsius to Kelvin Convert 100 o C to K K = o C K = = 373 K
Going from Kelvin to Celsius Convert 310 K to o C o C = K – 273 o C = 310 – 273 = 37 o C
Thermal Energy  the total energy of the particles in a material  KE - movement of particles  PE - forces within or between particles due to position  depends on temperature, mass, and type of substance
 B - same temperature, more mass 200 mL 80ºC A 400 mL 80ºC B.
 measured in joules (J)  a transfer of energy.
80ºC A 10ºC B  Heat flows from A to your hand = hot.  Heat flows from your hand to B = cold..
Insulators slow the transfer of heat due to air pockets. Conductors easily allow the transfer of heat, like metals. Heat is transferred by conduction, convection, and radiation..
Occurs best in solids. Heat continues to be transferred until both objects reach the same temperature, called a thermal equilibrium..
The cause of wind and weather..
Transferred in all directions. No contact required. Dark or dull objects absorb more than light or shiny objects do..
of 1 kg of material by 1 degree Kelvin  units: J/(kg·K) or J/(g·°C).
50 g Al50 g Cu Al - It has a higher specific heat. Al will also take longer to cool down..
Heat Transfer Q = m   T  C p Q:heat (J) m:mass (g)  T:change in temperature (K or °C) C p :specific heat (J/g·K or J/g.o C)  T = T f - T i – Q = heat loss + Q = heat gain
Heat Transfer Calorimeter  device used to measure changes in thermal energy Coffee cup Calorimeter  in an insulated system, heat gained = heat lost
How much heat is lost by the spoon. GIVEN: m = 32 g T i = 60°C T f = 20°C Q = . C p = 235 J/kg·K WORK: Q = m·  T·C p m = 32 g = kg  T = 20°C - 60°C = – 40°C  T = 293 K – 333 K = -40 K Q = (0.032kg)(-40 K)(235J/kg·K) Q = J (lost heat, negative).
GIVEN: m = 230 g T i = 12°C T f = 90°C Q = . C p = J/g· o C WORK: Q = m·  T·C p m = 230 g  T = 90°C - 12°C = 78°C Q = (230 g)(78 o C)(4.184 J/g· o C) Q = 75,061 J (gained heat, positive).

Heat Transfer

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