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Think-pair-share. Respond to at least One question below using the organizer provided. Be prepared to share your thoughts QUESTIONS: 1. Describe what happens to a rat that has been eaten by a python. 2. What is the function of the digestive system? What are calories?

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think pair share
Think-pair-share
  • Respond to at least One question below using the organizer provided. Be prepared to share your thoughts
  • QUESTIONS:
  • 1. Describe what happens to a rat that has been eaten by a python.
  • 2. What is the function of the digestive system? What are calories?
  • 3.How can you measure the calories contained in food?
  • 4. What do you think happens if a person eats more calories than their body needs?
thermochemistry

THERMOCHEMISTRY

http://ca.pbslearningmedia.org/resource/nvsn6.sci.bio.fuel/food-is-fuel/

swbat
SWBAT…..
  • define the terms system and surroundings in the context of a chemical reaction.
  • identify the system and surroundings in a thermochemicalreaction.
  • describe how heat is transferred in endothermic and exothermic reactions
  • Calculate specific heat of a substance in calories and joules
  • Calculate enthalpy changes in a thermochemicalrtn
  • Apply Hess’s law of heat summation in a thermochemical equation.
heat and work
Heat and Work:
  • TERMINOLOGIES:
  • Thermochemistry: studies energy changes in chemical reactions and changes of state.
  • Heat (q): is the transfer of energy from one object to another because of temperature difference (warmer to cooler object)
  • System: part of the universe being studied or focus of attention (e.g. reactants and products of a reaction)
  • Surroundings: the immediate vicinity of the system (e.g. container, space, universe, e.t.c.)
  • Law of conservation of energy: states that energy is neither created nor destroyed in any chemical or physical process.
exothermic and endothermic processes
Exothermic and EndothermicProcesses
  • COMPARE AND CONTRAST USING VENN DIAGRAM
  • Exothermic Process:
    • Heat is release to the surroundings (surroundings warms up)
    • The system loses heat (system products cools down)
    • q= negative
  • Endothermic Process:
    • Heat is absorbed from the surroundings (surroundings cool down)
    • The system gains heat (system products warms up)
    • q= positive
unit for measuring heat flow
Unit for Measuring Heat Flow
  • Calorie (cal) : quantity of heat needed to raise the temperature of 1g of pure water to 10C.
    • 1 Calorie = 1 Kilocalorie = 1000 calories
    • 20 Cal (dietary potential energy) = 20 Kcal (when energy completely used up/released)
  • Joules (S.I. Unit of energy)
    • One Joule (1J) of heat is the energy needed to raise the temperature of 1g of pure water to 0.23900C
    • Unit Conversion:
    • 1J = 0.2390 cal 4.184J = 1cal
    • 1000J = 1kJ (kiloJoules)
heat capacity
Heat Capacity
  • Heat Capacity: amount of heat needed to increase the temperature of an object to exactly 10C. ( Unit for heat capacity = J/0C)
  • Heat capacity depends on:
    • Mass of an object
    • Chemical composition of the object
  • Specific Heat Capacity (C): is the amount of heat it takes to raise the temperature of 1g of substance (object) to 10C. (Unit for Specific Heat = J/(g.0C) or J/(kg.0C) or kcal/(kg.0C) ). Remember: 1000g = 1Kg
check for understanding
Check for understanding
  • Thumbs Up
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  • What is your level of understanding on:
        • System and surroundings
        • Endothermic and Exothermic
        • Calorie/Kilocalorie
        • Heat Capacity
        • Specific Heat Capacity
calculating specific heat capacity c of a substance
Calculating Specific Heat/Capacity(C) of a Substance
  • Formula for calculating Specific Heat
  • Unit for Specific Heat
  • Specific Heats of some common substances (see PHC: table 17.1, page 508)
heat math problems
Heat Math problems
  • When 435J of heat is added to 3.4g of olive oil at 210C, the temperature increases to 850C. What is the specific heat of the olive oil?
  • How much heat is required to raise the temperature of 250.0g of mercury 520C?
  • An orange contains 445kJ of energy. What mass of water could the same amount of energy raise from 25.00C to the boiling point?
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