Chapter 9 Heat
Heat Temperature and Thermal Equilibrium Defining Heat Changes in Temperature and Phase
Temperature
Temperature and Kinetic Energy Temperature = A measure of the average kinetic energy of the particles in a substance For monatomic gas translational KE
For polyatomic substances…
Internal Energy Internal energy (U) = the total energy of a substance due to the KE and PE of its particles Internal energy depends on mass and temperature For an ideal gas, internal energy is proportional to just temperature
Temperature & Internal Energy Distinguish between temperature and internal energy Which depends on mass? Compare T and U for… 1 cup of water @ 20°C and 1 cup of water @ 25°C 1 cup of water @ 20°C and ½ cup of water @ 20°C 1 cup of hot tea and a swimming pool of cold water
Thermal Equilibrium Thermal equilibrium = the state in which two bodies in physical contact with each other have identical temperatures
Thermal Expansion Generally, at constant pressure, an increase in temperature causes an increase in volume Exception? Compare gases, liquids, and solids
Temperature Units Celsius (°C) Fahrenheit (°F) Kelvin (K)
Another important point to know: Absolute zero = 0 K
Temperature Conversions 𝑇F= 9 5 𝑇C+32.0 𝑇=𝑇C+273.15 𝑇F = Fahrenheit temperature 𝑇C = Celsius temperature 𝑇 = Kelvin temperature
Heat Heat = the energy transferred between objects because of a difference in their temperatures Energy transferred as heat moves from an object with higher temperature to an object with lower temperature
What is happening on a macroscopic scale? What is happening on a microscopic scale? (What is happening with temperature, internal energy, and heat?)
Heat = Q
3 Types of Heat Conduction Convection Radiation Requires contact Consider conductivity Convection Fluid movement Radiation Electromagnetic waves
Conservation of Energy Δ𝐾𝐸+Δ𝑃𝐸+Δ𝑈=0
Specific Heat Capacity Specific heat capacity = the quantity of heat required to raise 1 kg of a substance by 1 K or 1°C given constant pressure and volume Units: J/kg·°C 𝑐 𝑝 = 𝑄 𝑚Δ𝑇
Calorimetry = an experimental procedure used to measure the energy transferred from one substance to another as heat
𝑄 𝑤 =− 𝑄 𝑥 𝑐 𝑝,𝑤 𝑚 𝑤 Δ 𝑇 𝑤 =− 𝑐 𝑝,𝑥 𝑚 𝑥 Δ 𝑇 𝑥 energy absorbed by water energy released by substance = 𝑄 𝑤 =− 𝑄 𝑥 𝑐 𝑝,𝑤 𝑚 𝑤 Δ 𝑇 𝑤 =− 𝑐 𝑝,𝑥 𝑚 𝑥 Δ 𝑇 𝑥 Compare the final temperatures of the water and the substance
Latent Heat Latent heat (L) = the energy per unit mass that is transferred during a phase change of a substance Latent heat 𝑄=𝑚𝐿 Heat of fusion Solid/liquid 𝐿 𝑓 Heat of vaporization Liquid/gas 𝐿 𝑣