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Ch. 11

Ch. 11 . Thermochemistry. Unit 9 Vocabulary. Thermochemistry - concerned with heat changes that occur during chemical reactions Energy - capacity of an object to do work or produce heat Kinetic energy - the energy an object has due to its motion Potential energy - stored energy

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Ch. 11

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  1. Ch. 11 Thermochemistry

  2. Unit 9 Vocabulary • Thermochemistry - concerned with heat changes that occur during chemical reactions • Energy- capacity of an object to do work or produce heat • Kinetic energy- the energy an object has due to its motion • Potential energy- stored energy • Temperature- describes amount of motion of particles

  3. Unit 9 Vocabulary • Heat - describes amount of energy transferred from one object to another • Endothermic process- heat absorbing process • Exothermic process- heat releasing process • Specific heat- Amount of heat it takes to raise 1g of a substance by 1°C

  4. The Flow of Energy Heat is transferred from one object to another.

  5. Cranking up the Heat: Basic Thermodynamics • Energy is required in all biological and chemical processes.

  6. Kinetic Energy • the energy an object has due to its motion Potential Energy • stored energy

  7. Energy in the universe is constant, though it changes forms. Law of Conservation of energy – energy can neither be created nor destroyed

  8. Heat vs. Temperature • Temp. and heat are not the same thing. • Temp. describes amount of motion of particles • Heat describes amount of energy transferred from one object to another

  9. Describing Energy Changes Heat flow is from the warmer to the cooler object Heat Flow Heat Flow

  10. Describing Energy Changes Hot day 50°C = 122°F Energy transferred from fire to beans. Change in energy for beans would be positive. Beans lost energy, it was transferred to its surroundings. This change of energy for the beans would be negative,(change = ∆)

  11. Endothermic reactions – absorbs heat, ∆E is positive, the surroundings cool down Exothermic reactions – releases heat, ∆E is negative, the surroundings heat up Describing Energy Changes Surroundings Heat Surroundings Heat

  12. Units used to describe Energy: calorie – called “little calorie” – (cal) kilocalorie – called “Big calorie”- (CAL) 1000 calories – same as a food calorie Joule – the SI unit of heat - (J)

  13. CONVERSION FACTOR 1 cal = 4.184 joules 1 cal 4.184 J 4.184 J 1 cal

  14. Heat Units: Conversion Problems 1. Convert 32.7 cal to joules. 2. Convert 6.24 J to cal.

  15. Specific Heat - Amount of heat it takes to raise 1g of a substance by 1°C Metals have a low specific heat Water has a high specific heat

  16. Learning Check 1. On a sunny day, the concrete deck around an outdoor swimming pool becomes hot, while the water stays cool. This is because… A. The deck has a higher specific heat than the water B. The deck has a lower specific heat then the water C. Both objects have the same specific heat

  17. Learning Check 2. Two objects are sitting next to each other in the sunlight. Object A gets hotter than object B. A. Object A has a lower specific heat than object B B. Object A has a higher specific heat than object B C. Both objects have the same specific heat

  18. Specific Heat of Water 4.18 J/g ×°C or 1 cal/g ×°C Matches definition: Amount of heat it takes to raise 1g of a substance by 1°C

  19. Formula for Specific Heat q = amount of heat – measured in cal or J m = mass – measured in g C = specific heat – units are J/g x °C or cal/g x °C ΔT = change in temp – measured in °C q = mc ΔT

  20. Specific Heat Problems: 1. Aluminum has a specific heat of 0.9020 J/g × °C. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0°C to a temperature of 22.0°C?

  21. Specific Heat Problems: 2. 850 calories of heat are applied to a 250 g sample of liquid water with an initial temperature of 13.0 °C.  Find: a) the change in temperature and b) the final temperature.  (remember, the specific heat of liquid water, in calories, is 1.00 cal/g x °C.)

  22. 3. The temperature of a sample of water increases by 69.5 °C when 24,500 J are applied.  The specific heat of liquid water is 4.18 J/g x °C.  What is the mass of the sample of water? Specific Heat Problems:

  23. Specific Heat Problems: 4. When 34,700 J of heat are applied to a 350 g sample of an unknown material the temperature rises from 22.0°C to 173.0°C.  What must be the specific heat of this material?

  24. Energy and Change of State When energy is added to a solid substance, its temperature increases until its melting point is reached. Upon the addition of more energy, the substance begins to melt.  The temperature remains the same until all the substance has melted. ****

  25. Energy required to melt 1 gram of a substance at its melting point Enthalpy of Fusion (DHfus) Heating Curve: ( For Water) Temp DHfus Melting point (°C) 0 -10 Heating Ice (solid) -20 Time

  26. After the substance melts and if heating continues, the temperature will continue to rise until it reaches its boiling point. ۞The temperature remains the same until all the substance has boiled.*** Energy and Change of State

  27. Enthalpy of Vaporization (DHvap) Boiling Point 100 DHfus DHvap Temp Heating Water (liquid) Melting Point 0 (°C) -10 Heating Ice -20 Time Energy required to vaporize 1 gram of a substance at its boiling point

  28. ► Important Formulas to Know ◄ When a substance is being heated, use the following formula: q = (m)(c)(DT) When a substance is melting or boiling, use the following formula: q = (m) (DHfus or DHvap)

  29. q = (m)(c)(DT) (C) = Specific Heat: - of ice = 2.06 J/g x °C - of water = 4.18 J/g x °C - of steam = 2.02 J/g x °C

  30. q = (m) (DHfus or DHvap) Enthalpy Values for Water: DHfus = 334 J/g DHvap = 2260 J/g

  31. Learning Check:

  32. Sample Problem How much energy is required to convert 40g of ice at -10°C to steam at 150°C ? Use Both Formulas Draw a graph

  33. Sample Problem #1 How much heat is required to melt 5.67g of ice? Q = (m)(ΔH fus) Q = (5.67g)(334 J/g) Q =

  34. Sample Problem #2 How much energy is required to boil 85g of water?

  35. Sample Problem #3 How much energy is required to raise the temperature of 25g of water from 15°C to 75°C ?

  36. Sample Problem #4 What is the final temperature when 1250 J of energy is added to 15g of water at 25°C ?

  37. Practice How much energy is required to boil 50 grams of water? What is the final temperature when 2500 J of heat is added to 35 grams of water at 15 degrees Celsius?

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