ENDING my life (thermochem)

yikes

+q

endothermic

-q

exothermic

heat is added to the system

endothermic (+q)

feels cold (assume beaker)

endothermic (+q)

system gains energy

endothermic (+q)

ice cube melting

endothermic (+q)

cold packs

endothermic (+q)

surroundings are colder

endothermic (+q)

boiling water

endothermic (+q)

heat moves from the system to the surroundings

exothermic (-q)

heat is removed from the system

exothermic (-q)

feels hot (assume beaker)

exothermic (-q)

system loses energy

exothermic (-q)

burning fire

exothermic (-q)

heat goes from the system to the surroundings

exothermic (-q)

surroundings heat up (/get warmer)

exothermic (-q)

freezing water

exothermic (-q)

condensing steam

exothermic (-q)

Calorimetry

Measurement of heat flow

formula for heat

q = Cpm(Tf-Ti)

SI (metric) unit for energy

Joule (J, kilojoule = kJ)

Heat

The energy transferred between two systems at different temperatures that are in contact

Antoine Lavoisier

Father of “heat”

Thermodynamics

The study of energy and its transformations

Temperature

measure of the average motion (KE) of atoms/molecules in a system

temperature is… (intensive/extensive)?

intensive

Zeroth law

Objects that are in thermal equilibrium have the same temperature

First law

Energy cannot be created nor destroyed

q represents..

heat (J)

Cp represents..

specific heat (J/g°C)

m represents..

mass (g)

T_f represents..

the final temperature (°C)

T_i represents…

initial temperature (°C)

(Tf-Ti) can be simplified by..

just taking the change in temperature if stated in the problem

Enthalpy

a measure of the total energy of a thermodynamics system

△H = q

Enthalpy

another unit for heat

1 cal (food is 10³ cal)

heat flows through…..?

molecular collisions

1 J = _ kgm²/s²

1 kgm²/s²

KE = …?

KE = 1/2mv²

Heat Capacity

measures the heat energy required to raise the temperature of an entire object by 1°C (J/°C OR J/K)

Why is specific heat C_p?

C represents the heat, the subscript p tells us its at constant pressure

phase change from solid to liquid

melting —> endothermic

phase change from liquid to gas

vaporization —> endothermic

phase change from gas to liquid

condensation —> exothermic

phase change from liquid to solid

freezing —> exothermic

phase change from solid to gas

sublimation —> endothermic

phase change from gas to solid

deposition —> exothermic