Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
8th Edition
ISBN: 9780134421377
Author: Charles H Corwin
Publisher: PEARSON
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Question
Chapter 11, Problem 36E
Interpretation Introduction
Interpretation:
The amount of heat that is released while freezing
Concept introduction:
When a substance change its state from solid to liquid, then the amount of heat needed to melt
The heat of fusion for water is
When the state of water changes from liquid to solid, the same amount of heat energy is released and this heat change is known as heat of solidification
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Calculate the heat released when freezing 25.0 g of water at 0 °C.
Calculate the heat change in joules for freezing 235 gg of water at 0 ∘C∘C.
How much energy is given off when 563.8 g of NaCl solidifies at its freezing point of 801C ?
Chapter 11 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
Ch. 11 - Prob. 1CECh. 11 - Prob. 2CECh. 11 - Prob. 3CECh. 11 - Prob. 4CECh. 11 - Prob. 5CECh. 11 - Prob. 6CECh. 11 - Prob. 7CECh. 11 - Prob. 8CECh. 11 - Prob. 1KTCh. 11 - Prob. 2KT
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forwardCalculate the heat change in calories for freezing 45 gg of water at 0 ∘C∘C.arrow_forward2. Why does the temperature of a mixture of ice and water remain constant during melting and freezing?arrow_forward
- Calculate the heat lost by the liquid water (in kJ).arrow_forwardWhat is the enthalpy change when 1.00 g of water is frozen at 0⁰C?arrow_forwardGiven that a 10.0 g sample of ice at 0.0 °C melts and then the resultant water proceeds to warm to 20.0 °C, there are two separate processes (dealing with the transfer of heat) that describe that occurrence. What are those two processes?arrow_forward
- how many joules of heat are required to heat 25.0 g of ethyl alcohol from the prevailing room temperature, 22.5 oC , to its boiling point, 78.5oC?arrow_forwardCalculate the heat change in kilojoules for freezing 90.0 g of water at 0 ∘C.arrow_forwardCalculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °Carrow_forward
- A student wants to determine the melting point of water as part of an investigation into the strength of electrostatic forces. The student considers determining the freezing point of water instead. Is this a valid option? O No, it is not because the freezing point is not related to electrostatic forces. O No, it is not because the freezing point is not related to the melting point. O Yes, it is; and determining the freezing point is likely to be more accurate. O Yes, it is; but determining the freezing point is likely to be more difficult.arrow_forwardHow many joules of heat are required to heat 25.2 g of ethyl alcohol from the prevailing room temperature, 22.5 oC, to its boiling point, 78.5 oC?arrow_forwardAt what temperature does water freeze in kelvin? 100 K O 273 K O OKarrow_forward
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