Plan and Solve What unknown are you trying to calculate? Amount of energy absorbed, Q What formula contains the given quantity and the unknown? Q = mcAT = mc(T-T₁) Substitute the known values and solve. Q=(25.0 g)(0.48 cal/g-°C)(0.0°C - (-10.0°C)) = 120 cal Look Back and Check Is your answer reasonable? Yes, the sign shows that heat was absorbed and the unit, c proper unit for energy. Math Practice Note that
Plan and Solve What unknown are you trying to calculate? Amount of energy absorbed, Q What formula contains the given quantity and the unknown? Q = mcAT = mc(T-T₁) Substitute the known values and solve. Q=(25.0 g)(0.48 cal/g-°C)(0.0°C - (-10.0°C)) = 120 cal Look Back and Check Is your answer reasonable? Yes, the sign shows that heat was absorbed and the unit, c proper unit for energy. Math Practice Note that
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
Section: Chapter Questions
Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...
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![Initial temp
Plan and Solve
What unknown are you trying to calculate?
Amount of energy absorbed, Q
What formula contains the given quantity and the unknown?
Q = mcAT = mc(T₁-T₁)
Substitute the known values and solve.
Q=(25.0 g)(0.48 cal/g °C)(0.0°C - (-10.0°C)) = 120 cal
Look Back and Check
Is your answer reasonable?
Yes, the sign shows that heat was absorbed and the unit, calories, is a
proper unit for energy.
Math Practice
On a separate sheet of paper, solve the following problems. Note that quantity
of heat energy required to change the phase of a substance is given by the
following equation: Q = mL, where Q is the heat required, m is the mass, and
L is the heat of fusion or vaporization.
1. How much energy is absorbed when 25.0 g of ice at 0.0°C melts to form
water at 0.0°C? The heat of fusion of ice is 80 cal/g.
2. How much energy is absorbed when the water at 0.0°C in Question 1 is
heated to 100.0°C? The specific heat of water is 1.0 cal/g. °C.
3. How much energy is absorbed when the water at 100.0°C in Question 2
vaporizes to 100.0°C? The heat of vaporization of water is 540 cal/g.
4. The steam in Question 3 is used to melt ice. How much ice will be
melted by the energy released by the condensation of the steam at
100.0°C?
#4 ↑ please](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3570f510-88cc-47e8-8abe-e1329d4d401b%2F748f256e-0706-495f-b568-80d7eacb84ce%2Fj4zkfq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Initial temp
Plan and Solve
What unknown are you trying to calculate?
Amount of energy absorbed, Q
What formula contains the given quantity and the unknown?
Q = mcAT = mc(T₁-T₁)
Substitute the known values and solve.
Q=(25.0 g)(0.48 cal/g °C)(0.0°C - (-10.0°C)) = 120 cal
Look Back and Check
Is your answer reasonable?
Yes, the sign shows that heat was absorbed and the unit, calories, is a
proper unit for energy.
Math Practice
On a separate sheet of paper, solve the following problems. Note that quantity
of heat energy required to change the phase of a substance is given by the
following equation: Q = mL, where Q is the heat required, m is the mass, and
L is the heat of fusion or vaporization.
1. How much energy is absorbed when 25.0 g of ice at 0.0°C melts to form
water at 0.0°C? The heat of fusion of ice is 80 cal/g.
2. How much energy is absorbed when the water at 0.0°C in Question 1 is
heated to 100.0°C? The specific heat of water is 1.0 cal/g. °C.
3. How much energy is absorbed when the water at 100.0°C in Question 2
vaporizes to 100.0°C? The heat of vaporization of water is 540 cal/g.
4. The steam in Question 3 is used to melt ice. How much ice will be
melted by the energy released by the condensation of the steam at
100.0°C?
#4 ↑ please
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