![Introductory Chemistry (6th Edition)](https://www.bartleby.com/isbn_cover_images/9780134302386/9780134302386_largeCoverImage.gif)
Concept explainers
Interpretation: The amount of heat emitted during the condensation of
Concept introduction:
Heat of condensation is the amount of heat released to condense one mole of vapor into liquid.
Heat of condensation is opposite to the heat of vaporization. Since heat is released during condensation, condensation is an exothermic process. Hence, the value of heat of condensation is written with a negative sign.
The heat of condensation is used to calculate the amount of heat released to condense a given amount of liquid at a given temperature. For this, heat of condensation is used as a conversion factor between the amount of heat required to condense a liquid and moles of the liquid.
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 12 Solutions
Introductory Chemistry (6th Edition)
- 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_forwardIf you want to convert 56.0 g ice (at 0 °C) to water at 75.0 °C, calculate how many grams of propane, C3H8, you would have to bum to supply the energy to melt the ice and then warm it to the final temperature (at 1 bar).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_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?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_forward
- The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.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_forwardDraw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C s 2H2 g CH4 g Which is exothermic by 74.8 kJ/mol.arrow_forward
- How much heat, in joules and in calories, must be added to a 89.1 g chromium block with a specific heat of 0.450 J/g·°C to increase its temperature from 25°C to its melting temperature of 1907°C?arrow_forwardWhat is a phase change? Construct a heating-cooling curve for a substance that freezes at –23.0°C and has a boiling point of 67.0°C. Name all possible changes that can occur among the vapor, liquid, and solid phases of this substance, and name the four phase change enthalpies involved. Indicate whether these changes are exothermic or endothermicarrow_forwardHow much heat is required to convert 58.2g of liquid water at 15 °C to water vapor at 125 °C. (Use the constants given in the example above.) kJarrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxLiving By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningWorld of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College Div
![Text book image](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781938168390/9781938168390_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781559539418/9781559539418_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133958437/9781133958437_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781285199047/9781285199047_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780618562763/9780618562763_smallCoverImage.gif)