Energy Unit 1.

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Presentation transcript:

Energy Unit 1

States of Matter

Changing State of Matter

Changing States of Matter In order to go from 1 state of matter to another, it involves energy (usually heat energy- enthalpy) You are either removing the energy or adding more energy

Endothermic Processes How does heat move? From areas of higher temperature to lower temperature! Endothermic Processes Exothermic Processes Occur when heat is added to the system Examples Cooking Evaporation Instant cold packs Occur when heat is given off by the system Examples Instant heat packs Nuclear fission Candle burning

Exothermic or Endothermic?

What is HEAT? It’s the flow of energy due to a difference in temperature. From a higher temperature (higher kinetic energy) to a lower temperature (less kinetic energy) THERE IS NO SUCH THING AS COLD! It’s just the absence of heat! What is temperature? It’s the average amount of kinetic energy a substance has from its moving atoms/ molecules Kinetic energy is the energy of motion!

q = mCΔT Equation change in temperature, measured in °C ΔT = Tfinal – Tinitial heat energy – measured in joules (J) heat capacity – how much heat a substance can hold, measured in joules/gramdegrees Celsius mass - measured in grams (g)

Units for heat (q) Most food tells us the amount of energy in units of Calories. . . . Calories are kilocalories (1 Cal = 1000cal) The SI unit for energy is Joules (J) 1 cal = 4.184 J Let’s do some quick conversions.

How can you tell if a process is endothermic or exothermic? q is a positive number Why? The final temperature is higher than the initial temperature- we added heat to the system. ΔT = Tfinal – Tinitial q is a negative number Why? The final temperature is lower than the initial temperature- heat was given off from the system. ΔT = Tfinal – Tinitial Let’s solve some problems!