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.
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
INTRODUCTORY CHEMISTRY-W/SEL.SOLN.MAN.
- 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_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_forward
- Will 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_forwardThe enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.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 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_forwardHow 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_forwardA 31.0 g block of an unknown metal at 88.0°C was dropped into an insulated flask containing approximately 30.0 g of ice and 20.0 g of water at 0.0°C. After the system had reached a steady temperature, it was determined that 12.1 g of ice had melted. What is the specific heat of the metal? The heat of fusion of ice is equal to 334.166 J/g. a. 1.25 J/g°C b. 1.37 J/g°C c. 1.47 J/g°C d. 1.40 J/g°Carrow_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