Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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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?
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
20. 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
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Chapter 14 Solutions
Introductory Chemistry: A Foundation
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 - The energy required to melt 1 mole of a solid is...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 - Formaldehyde has the formula CH2O, where C is the...Ch. 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_forward3.) 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_forward
- The 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_forwardThe 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_forward
- Give me handwritten answerarrow_forwardWhat 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_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
- What is the enthalpy change in kJ for converting 5.0 mol of ice at -50.0°C to water at 70.0°C? The specific heats of ice, water, and steam are 2.09J/g"K, 4.18J/g*K and 1.84J/g"K, respectively. For H20, AH fus 6.01J and AHvap = 40.67J mal %3D molarrow_forward15) ) Liquid ammonia, NH,(1), was once used in home refrigerators as the heat transfer fluid. The specific heat capacity of the liquid is 4.7 J/gK and that of the vapor is 2.2 J/gK. The enthalpy of vaporization is 23.33 kJ/mol at the boiling point. If you heat 500 g of liquid ammonia from -40.0 °C to its boiling point of -33.3 °C, allow it to evaporate, and then continue warming to -5.0 °C, how much energy must you supply? t which que provide for make 400 g of solution t concentrated su concentratearrow_forwardA 22.5-g sample of ice at 0.0 oC is added to 100.0 g of warm water at 35.0 oC, and the final temperature of the mixture is 14.0 oC. (a)How much heat(in Joules)is lost by the warm water? (b) How much heat (in Joules) is absorbed by the melted ice when its temperature increases from 0.0 oC to 14.0 oC? (c) How much heat is absorbed by ice during melting at 0.0 oC? (d) What is the enthalpy of fusion of ice in kJ/mol? (Specific heat of water = 4.184 J/(g.oC)arrow_forward
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