Schaum's Outline of College Physics, Twelfth Edition (Schaum's Outlines)
12th Edition
ISBN: 9781259587399
Author: Eugene Hecht
Publisher: McGraw-Hill Education
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Question
Chapter 18, Problem 36SP
To determine
The heat of fusion of ice from the given data for ice at
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Check out a sample textbook solutionStudents have asked these similar questions
-1
Heat capacity of ice: 2090 J kg-¹ °C-1
Heat capacity of water (liquid): 4186 J kg-¹ °C-1
Latent heat of fusion: 3.36×105 J kg-¹
-1
Latent heat of vaporization: 2.26×107 J kg -1
Give your answers to at least three significant figures. Your answers must be accurate to 1%.
How much heat energy is required to raise the temperature of 625 g of ice from a temperature of -50 °C to a temperature of -27 °C?
J
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How much heat energy is required to raise the temperature of 625 g of water from a temperature of 43 °C to a temperature of 87 °C?
J
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How much heat energy is required to raise the temperature of 625 g of water (initially ice) from a temperature of -50 °C to a temperature of 87 °C?
J
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How much heat energy is required to evaporate 625 g of water which is initially at a temperature of 43 °C?
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A student obtains the following data in a calorimetry experiment designed to measure the specific heat of aluminum.
Initial temperature of water and calorimeter 70.3°C
Mass of water
0.402 kg
Mass of calorimeter
0.04 kg
Specific heat of calorimeter
0.60 kJ/kg.°C
Initial temperature of aluminum
Mass of aluminum
Final temperature of mixture
(a) Use these data to determine the specific heat of aluminum.
J/kg. °C
(b) Is your result within 15% of 900 J/kg . °C?
Yes
No
Need Help?
26.8°C
0.199 kg
66.4°C
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Measurement of specific heat of metals
Aluminum
Cupper
Mass of inner cup of calorimeter mcal, g
50
50
Specific heat of calorimeter Ccal, cal/(g °C)
Specific heat of water Cw, cal/(g °C)
0.217
0.217
1.00
1.00
Mass of metal Mm, g
80
140
Mass of inner cup + water mcal + Mw, g
220
240
Mass of water Mw, g
170
190
Initial temperature of calorimeter and water to, °C
Initial temperature of metal tm, °C
22
22
100
100
Final equilibrium temperature tr, °C
30
26
Thermal energy gain by calorimeter and water Qgain, cal
Specific heat of metal Cm, cal/(g °C)
Standard specific heat of metal Cst , cal/(g °C)
0.217
0.093
|% error
Thermal energy lost = Thermal energy gained
Thermal energy Q = cmAt
%3D
%3D
Specific heat C
|Thermal energy lost by metal = Thermal energy gained by (water + calorimeter)
%3D
EmMm(tm-tf)=(ccatMeat +CwMw)(tp- to)
%3D
(Ccaimcal+ Cymw)(tf- to).
Gm =
%3D
Mm(tm - t;)
|
Chapter 18 Solutions
Schaum's Outline of College Physics, Twelfth Edition (Schaum's Outlines)
Ch. 18 - 18.19 [I] Victoria Falls on the Zambezi River is...Ch. 18 - Prob. 20SPCh. 18 - 21. How much energy must be removed from a 10.0-kg...Ch. 18 - 22. A 100-kg chunk of ice at −150 °C is to have...Ch. 18 - Prob. 23SPCh. 18 - 24. A molten 50.0-kg quantity of gold at 1063 °C...Ch. 18 - Prob. 25SPCh. 18 - Prob. 26SPCh. 18 - Prob. 27SPCh. 18 - 18.28 [II] What will be the final temperature if...
Ch. 18 - Prob. 29SPCh. 18 - 18.30 [II] How long does it take a 2.50-W heater...Ch. 18 - 18.31 [II] A 55-g copper calorimeter contains 250...Ch. 18 - Prob. 32SPCh. 18 - 18.33 [II] How much heat is required to change 10...Ch. 18 - 18.34 [II] Ten kilograms of steam at 100 °C is...Ch. 18 - 18.35 [II] The heat of combustion of ethane gas is...Ch. 18 - Prob. 36SPCh. 18 - 18.37 [II] Determine the result when 100 g of...Ch. 18 - 18.38 [II] Determine the result when 10 g of steam...Ch. 18 - Prob. 39SPCh. 18 - 18.40 [II] How long will it take a 500-W heater to...Ch. 18 - Prob. 41SPCh. 18 - 18.42 [II] On a certain day the temperature is 20...Ch. 18 - 18.43 [II] How much water vapor exists in a 105-...Ch. 18 - 18.44 [II] Air at 30 °C and 90 percent relative...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, physics and related others by exploring similar questions and additional content below.Similar questions
- Beryllium has roughly one-half the specific heat of water (H2O). Rank the quantities of energy input required to produce the following changes from the largest to the smallest. In your ranking, note any cases of equality, (a) raising the temperature of 1 kg of H2O from 20C to 26C (b) raising the temperature of 2 kg of H2O from 20C to 23C (c) raising the temperature of 2 kg of H2O from 1C to 4C (d) raising the temperature of 2 kg of beryllium from 1C to 2C (e) raising the temperature of 2 kg of H2O from -1C to 2Carrow_forwardObject A is placed in thermal contact with a very large object B of unknown temperature. Objects A and B are allowed to reach thermal equilibrium; object Bs temperature does not change due to its comparative size. Object A is removed from thermal contact with B and placed in thermal contact with another object C at a temperature of 40C. Objects A and C are of comparable size. The temperature of C is observed to be unchanged. What is the temperature of object B?arrow_forwardCompare the SI units of specific heat and latent heat and explain any differences.arrow_forward
- The specific heat of substance A is greater than that of substance B. Both A and B are at the same initial temperature when equal amounts of energy are added to them. Assuming no melting or vaporization occurs, which of the following can be concluded about the final temperature TA of substance A and the final temperature TB of substance B? (a) TA TB (b) TA TB (c) TA = TB (d) More information is needed.arrow_forwardHow much thermal energy/heat is required to raise 2.3 kg of lead from 300°C to 1800°C? Use Table 1 p281 and Table 1 p291 to help you. O 1.8 x 10°J O 2. 5 x 10°J O8.2 x 10³J O4.5 x 10°J x 10°Jarrow_forwardAsaparrow_forward
- At atmospheric pressure, how much energy is required to heat 47.0 g of H2O(s) at -10.0◦C to H2O(g) at 129.0◦C? specific heat ice - 2093 J/kg C latent heat of fusion - 334*10^3 J/kg specific heat water - 4184 J/kg C latent heat of vaporization - 2260*10^3 J/kg specific heat vapor - 2010 J/kg C These values are approximate and fine to use. Please show all work.arrow_forwardFOLLOWING CONSTANTS ARE GIVEN FOR CALCULATIONS Specific Heat of Water = 4186 J/kg °C, Specific Heat of Iron = 452 J /kg °C, Specific Heat of Ice = 2093 J/kg °C, Specific Heat of Lead = 130 J/kg °C Latent Heat of Fusion = 3.34 x 105 J/kg, Specific Heat of Copper = 385.1 J /kg.°C Density of iron = 7.874 g /cm3 Density of copper = 8.95 g /cm3 1. A cylindrical shape iron object of radius 400000 µm and length 2 m initially at 30 °C is placed in hot water at 60 °C. Calculate the heat energy received by the iron ball.arrow_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 5.00 grams of ice at –15.0 °C is mixed with 40.0 grams of water at 75.0 °C? Multiple Choice 57.0 °C 28.3 °C 20.9 °C 18.6 °C 16.1 °C Carrow_forward
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