Reaction Energy

Specific Heat u The specific heat of any substance is the amount of heat required to raise the temperature of one gram of that substance by one degree Celsius. u Because different substances have different compositions, each substance has its own specific heat.

Exothermic and Endothermic Exothermic: Heat flows out of the system (to the surroundings). The value of ‘q’ is negative. Endothermic: Heat flows into the system (from the surroundings). The value of ‘q’ is positive.

Specific Heat q = m C p ΔT q = heat (J) C p = specific heat (J/(g. ° C) m = mass (g) Δ T = change in temperature = T f – T i ( ° C)

Measuring Heat u Heat changes that occur during chemical and physical processes can be measured accurately and precisely using a calorimeter. u A calorimeter is an insulated device used for measuring the amount of heat absorbed or released during a chemical or physical process.

A coffee-cup calorimeter made of two Styrofoam cups.

Phase Changes Solid Liquid Gas Melting Vaporization CondensationFreezing

Liquid Sublimation Melting Vaporization Deposition Condensation Solid Freezing Gas

Latent Heat q = m H v H v = latent heat of vaporization (J/g) H f = latent heat of fusion (J/g) q = m H f

Energy and Phase Change u Heat of vaporization (H v ) is the energy required to change one gram of a substance from liquid to gas. u Heat of fusion (H f ) is the energy required to change one gram of a substance from solid to liquid.

Specific Heat Problem 1) The temperature of a sample of iron with a mass of 10.0 g changed from 50.4°C to 25.0°C with the release of 114 J heat. What is the specific heat of iron? q =∆TC iron m = (25.0 – 50.4 ) C iron = J/g°C

2) A piece of metal absorbs 256 J of heat when its temperature increases by 182°C. If the specific heat of the metal is J/g°C, determine the mass of the metal. m = 4.67 g Specific Heat Problem

3) If 335 g water at 65.5°C loses 9750 J of heat, what is the final temperature of the water? T f = 58.5 °C Specific Heat Problem

4) As 335 g of aluminum at 65.5°C gains heat, its final temperature is 300. ° C. Determine the energy gained by the aluminum. q = J Specific Heat Problem

5) How much heat does it take to melt 12.0 g of ice at 0  C? q =HfHf m 12.0(334) q = 4010 J Latent Heat Problem

6) How much heat must be removed to condense 5.00 g of steam at 100  C? q =HvHv m 5.00(2260) q = J Latent Heat Problem

7) If 335 J of heat are added to melting 5.00 g of gold, what is the latent heat of fusion for gold in J/g? L f = 67 J/g Latent Heat Problem

8) The latent heat of fusion for platinum is 119 J/g. Platinum absorbs 735 J of heat. What is the mass of platinum? m = 6.18 g Latent Heat Problem

HEATING AND COOLING CURVES

The heating curve has 5 distinct regions.

The horizontal lines are where phase changes occur. melting vaporization

During any phase change, temperature is constant. melting

Kinetic energy increases on any diagonal line, and potential energy increases on any horizontal line. melting

The melting point temperature is equal to the freezing point temperature. The boiling point is the same as the temperature where condensation takes place. melting

Use q = m C p Δ T for all diagonal lines. Use q = m H f for melting and q = m H v for boiling. melting

A cooling curve also has 5 distinct regions. melting

For a cooling curve, kinetic energy decreases on any diagonal line, and potential energy decreases on any horizontal line. melting

Heating/Cooling Curve Problem 9. What is the freezing point of the substance? FP = 5°C

melting Heating/Cooling Curve Problem 10. What is the melting point of the substance? MP = 5°C

melting Heating/Cooling Curve Problem 11. What is the boiling point of the substance? BP = 15°C

melting Heating/Cooling Curve Problem 12. What letter represents the temperature where the solid is being heated? A

melting Heating/Cooling Curve Problem 13. What letter represents the temperature where the vapor is being heated? E

melting Heating/Cooling Curve Problem 14. What letter represents the temperature where the liquid is being heated? C

melting Heating/Cooling Curve Problem 15. What letter represents the melting of the solid? B

melting Heating/Cooling Curve Problem 16. What letters show a change in kinetic energy? A, C and E

melting Heating/Cooling Curve Problem 17. What letter represents condensation? D

melting Heating/Cooling Curve Problem 18. What is the freezing point of this substance? 18. What is the melting point of this substance? 19. At what time do the particles of this sample have the lowest average kinetic energy? FP = 90°C

melting Heating/Cooling Curve Problem 19. At what time do the particles of this sample have the lowest average kinetic energy? 18. What is the melting point of this substance? 19. At what time do the particles of this sample have the lowest average kinetic energy? 16 min

melting Heating/Cooling Curve Problem 20. How many minutes does it take the substance to condense? 18. What is the melting point of this substance? 19. At what time do the particles of this sample have the lowest average kinetic energy? 4 min

melting Heating/Cooling Curve Problem 21. What is the temperature range for the substance to be a vapor? 150 <T < 205

Heating Curve for Water Section A: Ice is being heated to the melting to the meltingpoint. Section B: The ice is melting. Section C: Water is being heated to the boiling to the boilingpoint. Section E: Steam is being heated. Section D: Water is Boiling.

Heating Curve for Water Section A q = m C p q = m C p ΔT (solid) Section B q = mH f Section C q = m C p q = m C p ΔT (liquid) Section E q = m C p q = m C p ΔT (gas) Section D q = mH v

Solving Problems u For water: Heat Ice Below 0  C + Melt Ice At 0  C + Heat Water 0  C  C + Boil Water At 100  C + Heat Steam Above 100  C

Specific Heat and Latent Heat 22) How much heat does it take to heat 12 g of ice at – 6  C to 25  C water? Round to a whole number. You begin at ice below 0 °C. Note: The final temperature for this process cannot exceed 0 °C. q =∆TC ice m 12(2.05)(0 - – 6) q = 148 J

 How much heat does it take to heat 12 g of ice at – 6  C to 25  C water? Round to a whole number. Since the temperature needs to rise to 25 °C, you must melt the ice next. q =HfHf m 12(334) q = 4008 J Specific Heat and Latent Heat, cont.

 How much heat does it take to heat 12 g of ice at – 6  C to 25  C water? Round to a whole number. You now have water at 0 °C. The final temperature of the water should be 25 °C. q =∆TC water m 12(4.18)(25 - 0) q = 1254 J Specific Heat and Latent Heat, cont.

 How much heat does it take to heat 12 g of ice at – 6  C to 25  C water? Round to a whole number. Finally, add all of the q values together. q = q = 5410 J Specific Heat and Latent Heat, cont.

23) How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C? Round to a whole number. You begin with ice at 0 °C, so you should melt it first. q =HfHf m 35(334) q = J Specific Heat and Latent Heat

 How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C? Round to a whole number. You now have water at 0 °C. The final temperature of the steam is to be 150 °C. You must take the water to 100 °C before you can even convert it to steam. q =∆TC water m 35(4.18)( ) q = J Specific Heat and Latent Heat, cont.

 How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C? Round to a whole number. Now you have water at 100 °C. Convert this to steam. q =HvHv m 35(2260) q = J Specific Heat and Latent Heat, cont.

 How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C? Round to a whole number. You must now take the steam at 100 °C to 150 °C. q =∆TC ice m 35(2.02)( ) q = 3535 J Specific Heat and Latent Heat, cont.

 How much heat does it take to heat 35 g of ice at 0  C to steam at 150  C? Round to a whole number. Finally, add all of the Q values together. q = q = J 3535 Specific Heat and Latent Heat, cont.

24) How much heat does it take to convert 16.0 g of ice to water at 0  C? (5340 J) Specific Heat and Latent Heat

25) How much heat does it take to heat 21.0 g of water at 12.0  C to water at 75.0  C? (5530 J) Specific Heat and Latent Heat

26) How much heat does it take to heat 14.0 g of water at 12.0  C to steam at  C? (37400 J) Specific Heat and Latent Heat

Calorimetry u For calorimetry problems, use the equation: – m C p ΔT = m C p ΔT which is based on the law of conservation of energy. Heat lost equals heat gained.

27) 125 g of water at 25.6°C is placed in a foam-cup calorimeter. A 50.0 g sample of the unknown metal is heated to a temperature of 115.0°C and placed into the water. Both water and metal attain a final temperature of 29.3°C. Determine the specific heat of the metal. Calorimetry Problem

u 125 g of water at 25.6°C is placed in a foam-cup calorimeter. A 50.0 g sample of the unknown metal is heated to a temperature of 115.0°C and placed into the water. Both water and metal have attain a final temperature of 29.3°C. Determine the specific heat of the metal. Find the heat gained by the water. q =∆TC water m 125(4.18)(29.3 – 25.6) q = 1930 J

Since heat lost equals heat gained, determine the specific heat of the metal. q =∆TC metal m =(29.3 – 115.0) C metal = J/g°C u 125 g of water at 25.6°C is placed in a foam-cup calorimeter. A 50.0 g sample of the unknown metal is heated to a temperature of 115.0°C and placed into the water. Both water and metal have attain a final temperature of 29.3°C. Determine the specific heat of the metal.

28) You put 352 g of water into a foam- cup calorimeter and find that its initial temperature is 22.0°C. What mass of 134°C lead can be placed in the water so that the equilibrium temperature is 26.5°C? m = 477 g Calorimetry Problem

29) You put water into a foam-cup calorimeter and find that its initial temperature is 25.0°C. What is the mass of the water if 14.0 grams of 125°C nickel can be placed in the water so that the equilibrium temperature is 27.5°C? m = 58.0 g Calorimetry Problem