Given the following constants below, how much heat (in kJ) must be added to completely transform the block of ice at -8.00°C to ice at the melting point of water? * Cice 2100 J/(kg-C°) = 4190 L(ka:Co)

Given the following constants below, how much heat (in kJ) must be added to completely transform the block of ice at -8.00°C to ice at the melting point of water? * Cice 2100 J/(kg-C°) = 4190 L(ka:Co)

Physics for Scientists and Engineers: Foundations and Connections

1st Edition

ISBN:9781133939146

Author:Katz, Debora M.

Publisher:Katz, Debora M.

Chapter21: Heat And The First Law Of Thermodynamics

Section: Chapter Questions

Problem 31PQ: Consider the latent heat of fusion and the latent heat of vaporization for H2O, 3.33 105 J/kg and...

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Question

Consider a block of ice, with a mass of 2.00 k
and an initial temperature of -8.00°C.
Given the following constants
below, how much heat (in kJ)
must be added to completely
transform the block of ice at
-8.00°C to ice at the melting
point of water? *
Cice
2100 J/(kg-C°)
Cwater
4190 J/(kg-C°)
%3D
Lf
= 33.5 x 10* J/kg
Ly
= 22. 6 × 105 ]/kg
2.1
4.2
8.4
33.6
67
335
670
2,260
2,680
None of the above.

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