ThermodynamicsPg 130 #2, 3
2. a) From the blue cup to the yellow.b) The blue cup because it contains the most heat.
3. a) Thermal energy derived from gasoline combustion. The heat from the motor is released into the environment outside the car. The temp. of the car decreases while the outside temp. close to the increases slightly.
b) The sun emits radiation and thermal energy. It is gradually transmitted to the inside of the car, where the temp. increases.
c) The water heater contains electric elements (electric potential energy) at a high temperature that transmit heat to the water in the heater, causing the water temp. to increase. The electric elements only cool when the electric is turned off, otherwise they always receive energy and remain practically stable.
d) The sun emits radiation and thermal energy. The heat and light from the sun, passing through the lens of the magnifying glass, are transmitted to the paper, whose temperature increases until combustion occurs. The flame the heats the environment around the paper. Once the paper has burned, it's temperature decreases and the heat is released into the surrounding environment.
e) The sun's radiation and thermal energy heats the Earth's atmosphere during the day. At night, the heat is released into outer space, which is cold in the absence of the sun's radiation. Consequently, outer space heats up slightly.
Pg. 133 #1, 2, 3
1. a) Beaker, water and acid: all open systemsb) Six bottles of soft drinks: six closed systemsBox: open systemc) A hot water bottle full of water: closed system.d) A cylinder filled with nitrogen: isolated system.e) A neon tube: closed systemf) A reaction vessel filled with gas: closed system.Calorimeter: isolated system
2. a) Electric and light energyb) Potential and kinetic energyc) Chemical energyd) Nuclear energy
3. a) The temperature rises.b) The temperature falls.c) If it is perfectly isolated, the temperature should not change. However, such perfection is impossible and the temperature falls.d) The temperature will rise, but much less than for the water, since thermal agitation is transferred less well in air than water.
Pg. 137 #2, 4, 5, 6, 8, 9, 11, 12, 16
2. Q= -41 J
4. 3.3 J/(g C)
5. 24.4 deg C
6. 7 deg C
8. 1 x 10 ^-3 g ( 1.43 x 10^-3 g)
9. Since more energy is required to boil oil (38 kJ) than water (33 kJ), it is faster to boil a potato than fry it.
11. The strawberry pie will cool fastest since it releases the least heat. The quantity of heat of the strawberry pie (Qstrawberries) is the smallest. Qstrawberries= -5.625 x 10^4 (g C)
12. By comparing their heat capacities we see the heat released by the wood will be approx. two times greater than that released by the glass.
16. c=0.79 J/(g C)The value of the specific heat capacity that is closest to the answer is 0.84. Therefore, the substance is glass.
Pg. 141 #2, 4, 5, 7, 9, 11Refer to Pg. 134 for the specific heats of various substances to solve these problems
Answers Textbook Pg. 141
2. V = 941 L
4. 0.1654 J/g°C
5. Ti = - 8.3°C
7. Tf = -3.78°C
9. Tf = 1.712°C Answer: Yes, since the final temperature is above 0°C, the ice will melt 11. Final temperature = -113.45 deg C. The heat transfer from the ice to the nitrogen is -5.3 kJ
Read Pages 148-151Pg.
155 #1, 2, 3, 5 Read Pages 152-154Pg 155 #4, 6
Answers Textbook Pg. 155
1. a) endothermic
b) exothermic
c) exothermic
d) endothermic
e) exothermic
2. a) endothermic
b) exothermic
c) exothermic
d) exothermic
3. b)
4. Will post in class
5. a) 30°C
b) 10°C
c) -10 kJ/mol
d) 13 kJ/mol
6. a) 2Li(s) + 2HCl(g) →2LiCl(s) + H2(g) + 562 kJ Exothermic Reaction
2Li(s) + 2HCl(g) →2LiCl(s) + H2(g) ΔH = -562 kJ
b) 2NH3(g) + 2CO2(g) + 861kJ →C2H6(g) + 2NO2(g) Endothermic Reaction
2NH3(g) + 2CO2(g) + 861kJ →C2H6(g) + 2NO2(g) ΔH = 861 kJ
Extra worksheet for enthalpy diagrams, thermochemical reactions attached below
Thermo calculations
Pg. 162 #3, 4, 7, 8, 9, 10
Answers to Pg. 162
#3. -334 kJ
#4. 677.1 kJ
#7. 737.9 kJ
#8. +58.1 kJ/mol
#9. 24.3 g/mol (Magnesium)
#10. 128.5 g
Pg. 163# 13, 15, 16, 18
Answers:
#13 a) P4H10(s) +6H2O(l) → 4H3PO4(aq) + 64.3 kJb) 321.5 kJc) 38.6 kJ
#15 a) -244 kJ/molb) -318.03 kJ/molc) 81.60 kJ/mold) -372.8 kJ/mol
#16 652 kJ
#18 229 kJ
2. a) From the blue cup to the yellow.b) The blue cup because it contains the most heat.
3. a) Thermal energy derived from gasoline combustion. The heat from the motor is released into the environment outside the car. The temp. of the car decreases while the outside temp. close to the increases slightly.
b) The sun emits radiation and thermal energy. It is gradually transmitted to the inside of the car, where the temp. increases.
c) The water heater contains electric elements (electric potential energy) at a high temperature that transmit heat to the water in the heater, causing the water temp. to increase. The electric elements only cool when the electric is turned off, otherwise they always receive energy and remain practically stable.
d) The sun emits radiation and thermal energy. The heat and light from the sun, passing through the lens of the magnifying glass, are transmitted to the paper, whose temperature increases until combustion occurs. The flame the heats the environment around the paper. Once the paper has burned, it's temperature decreases and the heat is released into the surrounding environment.
e) The sun's radiation and thermal energy heats the Earth's atmosphere during the day. At night, the heat is released into outer space, which is cold in the absence of the sun's radiation. Consequently, outer space heats up slightly.
Pg. 133 #1, 2, 3
1. a) Beaker, water and acid: all open systemsb) Six bottles of soft drinks: six closed systemsBox: open systemc) A hot water bottle full of water: closed system.d) A cylinder filled with nitrogen: isolated system.e) A neon tube: closed systemf) A reaction vessel filled with gas: closed system.Calorimeter: isolated system
2. a) Electric and light energyb) Potential and kinetic energyc) Chemical energyd) Nuclear energy
3. a) The temperature rises.b) The temperature falls.c) If it is perfectly isolated, the temperature should not change. However, such perfection is impossible and the temperature falls.d) The temperature will rise, but much less than for the water, since thermal agitation is transferred less well in air than water.
Pg. 137 #2, 4, 5, 6, 8, 9, 11, 12, 16
2. Q= -41 J
4. 3.3 J/(g C)
5. 24.4 deg C
6. 7 deg C
8. 1 x 10 ^-3 g ( 1.43 x 10^-3 g)
9. Since more energy is required to boil oil (38 kJ) than water (33 kJ), it is faster to boil a potato than fry it.
11. The strawberry pie will cool fastest since it releases the least heat. The quantity of heat of the strawberry pie (Qstrawberries) is the smallest. Qstrawberries= -5.625 x 10^4 (g C)
12. By comparing their heat capacities we see the heat released by the wood will be approx. two times greater than that released by the glass.
16. c=0.79 J/(g C)The value of the specific heat capacity that is closest to the answer is 0.84. Therefore, the substance is glass.
Pg. 141 #2, 4, 5, 7, 9, 11Refer to Pg. 134 for the specific heats of various substances to solve these problems
Answers Textbook Pg. 141
2. V = 941 L
4. 0.1654 J/g°C
5. Ti = - 8.3°C
7. Tf = -3.78°C
9. Tf = 1.712°C Answer: Yes, since the final temperature is above 0°C, the ice will melt 11. Final temperature = -113.45 deg C. The heat transfer from the ice to the nitrogen is -5.3 kJ
Read Pages 148-151Pg.
155 #1, 2, 3, 5 Read Pages 152-154Pg 155 #4, 6
Answers Textbook Pg. 155
1. a) endothermic
b) exothermic
c) exothermic
d) endothermic
e) exothermic
2. a) endothermic
b) exothermic
c) exothermic
d) exothermic
3. b)
4. Will post in class
5. a) 30°C
b) 10°C
c) -10 kJ/mol
d) 13 kJ/mol
6. a) 2Li(s) + 2HCl(g) →2LiCl(s) + H2(g) + 562 kJ Exothermic Reaction
2Li(s) + 2HCl(g) →2LiCl(s) + H2(g) ΔH = -562 kJ
b) 2NH3(g) + 2CO2(g) + 861kJ →C2H6(g) + 2NO2(g) Endothermic Reaction
2NH3(g) + 2CO2(g) + 861kJ →C2H6(g) + 2NO2(g) ΔH = 861 kJ
Extra worksheet for enthalpy diagrams, thermochemical reactions attached below
Thermo calculations
Pg. 162 #3, 4, 7, 8, 9, 10
Answers to Pg. 162
#3. -334 kJ
#4. 677.1 kJ
#7. 737.9 kJ
#8. +58.1 kJ/mol
#9. 24.3 g/mol (Magnesium)
#10. 128.5 g
Pg. 163# 13, 15, 16, 18
Answers:
#13 a) P4H10(s) +6H2O(l) → 4H3PO4(aq) + 64.3 kJb) 321.5 kJc) 38.6 kJ
#15 a) -244 kJ/molb) -318.03 kJ/molc) 81.60 kJ/mold) -372.8 kJ/mol
#16 652 kJ
#18 229 kJ
Enthalpy Calculations Worksheet Ans
ex2: change in Temperature - 0.2 °C
ex 3: 70.55 g of NH4Cl needs to be added
ex4: 40 g of ethanol
ex2: change in Temperature - 0.2 °C
ex 3: 70.55 g of NH4Cl needs to be added
ex4: 40 g of ethanol
enthalpy_calculations.pdf | |
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thermodynamicsheatsofreactionworksheet.doc | |
File Size: | 36 kb |
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heat_transfer_ans.pdf | |
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