4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C? 5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to steam at 105.0 °C. How much heat would be released in the reverse process?
4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C? 5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to steam at 105.0 °C. How much heat would be released in the reverse process?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C?
5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to
steam at 105.0 °C. How much heat would be released in the reverse process?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0acb0c38-6b47-42a4-a20e-50bfbc809f8e%2Fed30b222-88c7-47d7-b317-ffe629f63228%2F1p6de1e_processed.png&w=3840&q=75)
Transcribed Image Text:4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C?
5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to
steam at 105.0 °C. How much heat would be released in the reverse process?
Expert Solution
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Step 1
The specific heat of water is 4.184 J/g °C. It is related with heat absorbed or evolved by system as -
Q = m c ∆T
Here,
Q = Heat evolved or absorbed by the system in Joules or kilojoule
m = mass of substance in gram or kilogram
c = specific heat of the substance in J/g °C or kJ/kg °C
∆T = change in temperature = T2 - T1 (T2 is final temperature and T1 is initial temperature of the system)
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