These answers following are wrong ANSWER 1: Deduction: -3% ANSWER 2: Deduction:
ID: 1568733 • Letter: T
Question
These answers following are wrong
ANSWER 1: Deduction: -3%
ANSWER 2: Deduction: -3%
.475
22.2
Exercise 17.41
A 5.40 kg piece of solid copper metal at an initial temperature T is placed with 2.00 kg of ice that is initially at -15.0 C . The ice is in an insulated container of negligible mass and no heat is exchanged with the surroundings. After thermal equilibrium is reached, there is 0.90 kg of ice and 1.10 kg of liquid water.
Part A
What was the initial temperature of the piece of copper?
Express your answer to three significant figures and include the appropriate units.
C
These answers following are wrong
ANSWER 1: Deduction: -3%
ANSWER 2: Deduction: -3%
T =.475
C T =22.2
CExercise 17.41
A 5.40 kg piece of solid copper metal at an initial temperature T is placed with 2.00 kg of ice that is initially at -15.0 C . The ice is in an insulated container of negligible mass and no heat is exchanged with the surroundings. After thermal equilibrium is reached, there is 0.90 kg of ice and 1.10 kg of liquid water.
Part A
What was the initial temperature of the piece of copper?
Express your answer to three significant figures and include the appropriate units.
T =C
Explanation / Answer
specific heat of ice = 2.09 kJ/kg·°C
So it takes 2.09*2*15 to raise the temperature of 2kg of ice by 22 degrees C to 0 degrees C.
= 62.7 kJ.
Latent heat of fusion (ice to water) is 334kJ/kg.
It takes 334*1.10 kJ to melt 1.10 kg of ice at 0 degrees C to water at 0 degrees C,
= 367.4 kJ.
So 5.4 kg of copper has lost (62.7 + 367.4) kJ of heat in falling from T degrees C to 0 degrees C,
Specific heat of copper = 0.385 kJ/kgC
So 430.1 kJ = 0.385*5.4*(T - 0)
430.1 = 2.079T
T = 430.1/2.079
T = 207 degrees C = Initial temperature of copper
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.