EBK INTRODUCTORY CHEMISTRY
8th Edition
ISBN: 9780100480483
Author: DECOSTE
Publisher: YUZU
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Textbook Question
Chapter 14.2, Problem 14.1SC
trong>Exercise 14.1 Calculate the total energy required to melt
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3. (a) How much heat must be absorbed by ice of mass m=800 g at -20°C to take it to the steam at 120°C
? Given the specific heat of ice is 2220 J/kg.K, specific heat of water is 4186 J/kg.K, specific heat of steam
is 1996 J/kg.K, the latent heat of fusion is 333 KJ/kg and latent heat of vaporization is 226 KJ/kg. (b) If we
supply the ice a total energy of only 310 KJ, what are the final state and temperature of the water?
15
Figure below shows the phase diagram of water.
А
„H
„F
„G
D
T
Fig. 7.1
(a)
(b)
Which curve represents the equilibrium between ice and water vapour?
State the phase changes when a sample at point E is heated at constant pressure
until point F is reached. (hint: draw and label new points in your diagram to
explain your answer)
Name the point at which the BC line intersects 1 atm line.
The BC line has a negative slope. Explain.
(c)
(d)
8.
4.) Benzene, C6H6, has a normal melting point of 5.5°C and a normal boiling point of 80.1°C. How much heat,in Joules, is required to convert a 54.68 gram sample of solid benzene at -30.0°C into to benzene vapor at atemperature of 120.0°C at a pressure of 1 atm? Some potentially useful physical data for benzene are:ssolid = 1.18 J/g∙°C; sliquid = 0.946 J/g∙°C; sgas = 1.05 J/g∙°C; ΔHfus = 9.95 kJ/mol; ΔHvap = 33.83 kJ/mol
Chapter 14 Solutions
EBK INTRODUCTORY CHEMISTRY
Ch. 14.2 - trong>Exercise 14.1 Calculate the total energy...Ch. 14.3 - Prob. 1CTCh. 14.6 - trong>Exercise 14.2 Name the type of crystalline...Ch. 14 - ou seal a container half-filled with water. Which...Ch. 14 - xplain the following: You add 100mLof water to a...Ch. 14 - Prob. 3ALQCh. 14 - Prob. 4ALQCh. 14 - Prob. 5ALQCh. 14 - Prob. 6ALQCh. 14 - Prob. 7ALQ
Ch. 14 - ow do the following physical properties depend on...Ch. 14 - ook at Fig. 14.2. Why doesn't temperature increase...Ch. 14 - Prob. 10ALQCh. 14 - Prob. 11ALQCh. 14 - Prob. 12ALQCh. 14 - Prob. 13ALQCh. 14 - Prob. 14ALQCh. 14 - Prob. 15ALQCh. 14 - True or false? Methane (CH4) is more likely In...Ch. 14 - Prob. 17ALQCh. 14 - Prob. 18ALQCh. 14 - Prob. 19ALQCh. 14 - Which would you predict should be larger for a...Ch. 14 - Prob. 21ALQCh. 14 - Prob. 22ALQCh. 14 - Prob. 23ALQCh. 14 - ases have (higher/lower) densities than liquids or...Ch. 14 - Prob. 2QAPCh. 14 - Prob. 3QAPCh. 14 - he enthalpy (H)of vaporization of water is about...Ch. 14 - Prob. 5QAPCh. 14 - Prob. 6QAPCh. 14 - Prob. 7QAPCh. 14 - Prob. 8QAPCh. 14 - Prob. 9QAPCh. 14 - Prob. 10QAPCh. 14 - Prob. 11QAPCh. 14 - What does the molar heat of fusion of a substance...Ch. 14 - The following data have ban collected for...Ch. 14 - The molar heat of fusion of aluminum metal is...Ch. 14 - Prob. 15QAPCh. 14 - Prob. 16QAPCh. 14 - The molar heats of fusion and vaporization for...Ch. 14 - It requires 113Jto melt 1.00gof sodium metal at...Ch. 14 - Consider the iodine monochloride molecule, ICI....Ch. 14 - Prob. 20QAPCh. 14 - Prob. 21QAPCh. 14 - Prob. 22QAPCh. 14 - Prob. 23QAPCh. 14 - Prob. 24QAPCh. 14 - What type of intermolecular forces is active in...Ch. 14 - Prob. 26QAPCh. 14 - Prob. 27QAPCh. 14 - The heats of fusion of three substances are listed...Ch. 14 - When dry ammonia gas (NH3)is bubbled into a...Ch. 14 - Prob. 30QAPCh. 14 - Prob. 31QAPCh. 14 - If you've ever opened a bottle of rubbing alcohol...Ch. 14 - Prob. 33QAPCh. 14 - Prob. 34QAPCh. 14 - Which substance in each pair would be expected to...Ch. 14 - Which substance in each pair would be expected to...Ch. 14 - Prob. 37QAPCh. 14 - Two molecules that contain the same number of each...Ch. 14 - Prob. 39QAPCh. 14 - Prob. 40QAPCh. 14 - How do ionic solids differ in structure from...Ch. 14 - A common prank on college campuses is to switch...Ch. 14 - Prob. 43QAPCh. 14 - What types of forces exist between the individual...Ch. 14 - Prob. 45QAPCh. 14 - Prob. 46QAPCh. 14 - Prob. 47QAPCh. 14 - Prob. 48QAPCh. 14 - Prob. 49QAPCh. 14 - Prob. 50QAPCh. 14 - Prob. 51APCh. 14 - Prob. 52APCh. 14 - Prob. 53APCh. 14 - Prob. 54APCh. 14 - Prob. 55APCh. 14 - Prob. 56APCh. 14 - Prob. 57APCh. 14 - Prob. 58APCh. 14 - Prob. 59APCh. 14 - Prob. 60APCh. 14 - Given the densities and conditions of ice, liquid...Ch. 14 - Prob. 62APCh. 14 - Which of the substances in each of the following...Ch. 14 - Prob. 64APCh. 14 - Prob. 65APCh. 14 - Prob. 66APCh. 14 - Prob. 67APCh. 14 - Prob. 68APCh. 14 - Describe, on both a microscopic and a macroscopic...Ch. 14 - Cake mixes and other packaged foods that require...Ch. 14 - Prob. 71APCh. 14 - Prob. 72APCh. 14 - The molar heat of vaporization of carbon...Ch. 14 - Prob. 74APCh. 14 - Prob. 75APCh. 14 - Prob. 76APCh. 14 - Prob. 77APCh. 14 - Prob. 78APCh. 14 - Prob. 79APCh. 14 - Prob. 80APCh. 14 - Prob. 81APCh. 14 - Prob. 82APCh. 14 - Prob. 83APCh. 14 - Prob. 84APCh. 14 - Describe in detail the microscopic processes that...Ch. 14 - Prob. 86APCh. 14 - Prob. 87APCh. 14 - Prob. 88APCh. 14 - Prob. 89APCh. 14 - Describe, on a microscopic basis, the processes of...Ch. 14 - Prob. 91APCh. 14 - Prob. 92APCh. 14 - Which of the following compound(s) exhibit only...Ch. 14 - Which of the following statements about...Ch. 14 - Prob. 95CPCh. 14 - Prob. 96CPCh. 14 - Prob. 97CPCh. 14 - Which of the following statements is(are) true?...
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- What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water at 100C is 40.66 kJ/mol.arrow_forwardRefer to the phase diagram below, and describe the phase changes (and the temperatures at which they occur) when CO2 is heated from -80° C to -20° C at (a) a constant pressure of 3 atm; (b) a constant pressure of 6 atm; (c) a constant pressure of 9 atmarrow_forward20. How much heat is required to convert 5.0 g of ice at -10.0 °C to liquid water at 15.0 'C? (Assume heat capacities are independent of temperature.) Enthalpy of fusion Specific heat capacity of ice Specific heat capacity of water (A) 4.2 X 10-J (C) 9.3 X 10³ J 6.00 kJ mol 37.8 J-mol C 76.0 Jmol. C (B) 2.1 x 10³ J (D) 3.8 x 10¹ J tacoarrow_forward
- 3.) How much heat (J) is required to convert a 90.10 g sample of ice at –45.0°C into to water at 0.0°C? Somepotentially useful physical data for water are: ssolid = 2.03 J/g∙°C; sliquid = 4.18 J/g∙°C; sgas = 1.99 J/g∙°C; ΔHfus =6.01 kJ/mol ; ΔHvap = 40.6 kJ/molarrow_forwardLl.123.arrow_forwardThe specific heat of ice is 2.100 kJ/kg °C, the heat of fusion for ice at 0°C is 333.7 kJ/kg, the specific heat of water 4.186 kJ/kg °C, and the heat of vaporization of water at 100.0°C is 2,256 kJ/kg. What is the final equilibrium temperature when 10.00 grams of ice at -15°C is mixed with 3.000 grams of steam at 100°C? 87.21°C 85.32°C 82.56°C 80.12°C 78.45°Carrow_forward
- The specific heat of ice is 2.10 kJ/kg∙°C, the heat of fusion for ice at 0°C is 333.7 kJ/kg, the specific heat of water 4.186 kJ/kg∙°C, and the heat of vaporization of water at 100°C is 2,256 kJ/kg. What is the final equilibrium temperature when 10.0 grams of ice at -15°C is mixed with 40.0 grams of water at 75°C?arrow_forwardhonen 15 12. Calculate the amount of heat needed to change 45.0 grams of ice at -25.0 °C to steam at 250.0 °C. (For water, AHfus = 333 J/g; AHvap = 2260 J/g; Specific Heat (ice) = 2.10 Jg¹ K-¹; Specific Heat (steam) = 2.00 J g-¹ K-¹) a. 14.7 kJ b. 33.7 kJ C. 116 kJ E d. 151 kJ e. 175 kJ Letter answer to question #12:arrow_forwardGive me handwritten answerarrow_forward
- What quantity of energy does it take to convert 0.700 kg ice at -20.°C to steam at 250.°C? Specific heat capacities: ice, 2.03 J/g °C; liquid, 4.2 J/g·°C; steam, 2.0 J/g·°C; \Hvap = 40.7 kJ/mol; \Hfus = 6.02 kJ/mol. kJ Energy = =arrow_forward(c) Is methane a solid, liquid, or gas at 1 atm and 0 °C? (d) If solid methane at 1 atm is heated while the pressure is held constant, will it melt or sublime? (e) If methane at 1 atm and 0 °C is compressed until a phase change occurs, in which state is the methane when the compression is complete?arrow_forwardFor water, specific heat values for the solid and liquid phase are 2.00 J/gC and 4.18 J/gC respectively andthe heat of vaporization and the heat of fusion are 2260 J/g and 334 J/g respectively How doesthe slope of the ∆T line for a phase diagra from solid and liquid compare for water? Explain the comparison interms ofspecific heat capacities.▪ How does the horizontal length of the melting/boiling portions of the graph compare for water? Explain the comparison in terms of IMFs.arrow_forward
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