7. Calculating required heats. You have samples of water to do informal experiments in your college dorm-room kitchen. You are using a powerful refrigerator to extract heat from water samples to reduce the temperature of the samples for research. You will need the following information: Specific heat of ice C; = 0.480 cal/(g-ºC); heat of fusion of water L₁ = 79.9 cal/g, and specific heat of water Cw = 1.00 cal/(g-°C). (a) The mass of a water sample is 11.16 g. Suppose the initial temperature of the water is 76.22 °C. How much heat is removed from the sample to convert the water into pure ice at -12.11 °C? (b) The mass of a water sample is 11.16 g. Suppose the initial temperature of the water is 76.22 °C. How much heat is removed in order to reduce the temperature of the water sample to freezing temperature and then freeze 75 % water of the water? In other words, three-fourths of the 11.16-g water sample is frozen into ice.
7. Calculating required heats. You have samples of water to do informal experiments in your college dorm-room kitchen. You are using a powerful refrigerator to extract heat from water samples to reduce the temperature of the samples for research. You will need the following information: Specific heat of ice C; = 0.480 cal/(g-ºC); heat of fusion of water L₁ = 79.9 cal/g, and specific heat of water Cw = 1.00 cal/(g-°C). (a) The mass of a water sample is 11.16 g. Suppose the initial temperature of the water is 76.22 °C. How much heat is removed from the sample to convert the water into pure ice at -12.11 °C? (b) The mass of a water sample is 11.16 g. Suppose the initial temperature of the water is 76.22 °C. How much heat is removed in order to reduce the temperature of the water sample to freezing temperature and then freeze 75 % water of the water? In other words, three-fourths of the 11.16-g water sample is frozen into ice.
Physics for Scientists and Engineers, Technology Update (No access codes included)
9th Edition
ISBN:9781305116399
Author:Raymond A. Serway, John W. Jewett
Publisher:Raymond A. Serway, John W. Jewett
Chapter20: The First Law Of Thermodynamics
Section: Chapter Questions
Problem 20.3OQ: Assume you are measuring the specific heat of a sample of originally hot metal by using a...
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Question
Please answer both questions
For question 5 only answer part b and c
Transcribed Image Text:7.
Calculating required heats. You have samples of water to do informal
experiments in your college dorm-room kitchen. You are using a powerful
refrigerator to extract heat from water samples to reduce the temperature of the
samples for research.
You will need the following information: Specific heat of ice C₁ = 0.480 cal/(g-°C); heat of
fusion of water L₁ = 79.9 cal/g, and specific heat of water Cw = 1.00 cal/(g-°C).
(a)
The mass of a water sample is 11.16 g. Suppose the initial temperature of
the water is 76.22 °C. How much heat is removed from the sample to convert the
water into pure ice at
-12.11 °C?
(b)
The mass of a water sample is 11.16 g. Suppose the initial temperature of
the water is 76.22 °C. How much heat is removed in order to reduce the temperature of
the water sample to freezing temperature and then freeze 75 % water of the water? In
other words, three-fourths of the 11.16-g water sample is frozen into ice.
Transcribed Image Text:5.
An outside stereo speaker at a ski resort emits sound
waves with a power output of 90.00 W and frequency 1000.00 Hz.
a.
At what distance from the speaker would you experience the sound
at exactly 111 dB?
DOPPLER EFFECT:
b.
Suppose a skier is traveling toward the speaker at speed 19.72 m/s.
What is the frequency heard by the skier?
C.
Suppose a skier is traveling away from the speaker at speed 19.65
m/s. What is the frequency heard by the skier?
d.
Compare the wavelengths of part b. and part c. Which wavelength
is larger, that of part b. or part c? Compute the magnitude of the difference
between the wavelengths in part b. and part c.
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