Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
8th Edition
ISBN: 9780134421377
Author: Charles H Corwin
Publisher: PEARSON
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Chapter 11, Problem 38E
Interpretation Introduction
Interpretation:
The amount of heat that is released to convert
Concept introduction:
When the state of water changes from liquid to solid, the amount of heat energy is released and this heat change is known as heat of solidification
The heat of solidification for water is
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Given 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?
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Calculate the heat lost by the liquid water (in kJ).
Chapter 11 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
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- The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.arrow_forwardWill a closed container of water at 70 C or an open container of water at the same temperature cool faster on a cold winter day? Explain why.arrow_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forward
- The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.arrow_forwardA quantity of ice at 0C is added to 64.3 g of water in a glass at 55C. After the ice melted, the temperature of the water in the glass was 15C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g C).arrow_forward1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)arrow_forward
- Which requires the absorption of a greater amount of heat—vaporizing 100.0 g of benzene or boiling 20.0 g of water? (Use Table 8.2.)arrow_forward9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?arrow_forwardDefine the joule in terms of SI base units.arrow_forward
- The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?arrow_forwardMelting lead requires 5.50 cal/g. Calculate how many joules are required to melt 1.00 lb (454 g) lead.arrow_forwardCalculate the heat released when 65.5g of water at 55.5 ° C cools to ice at 0.0 ° C. (Given that the specific heat of liquid water is 1.00 calg×°C, and heat of water solidification is 80.0 cal/g.).arrow_forward
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