Concept explainers
(a)
Interpretation:
The phase change in iodine sample when temperature is held at
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure on a phase diagram at which gas, liquid, and solid phases coexist is called triple point. The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
Conversion of liquid into gas is called vaporization. Conversion of solid into liquid or vice-versa is called melting or fusion. Conversion of solid into gas is called sublimation.
(b)
Interpretation:
The phase change in iodine sample when the temperature is reduced from
Concept introduction:
Phase diagram is a graph that represents the solid phase, liquid phase, and gaseous phase of one substance or mixture of substance under different states of temperature and pressure.
The temperature and pressure on a phase diagram at which gas, liquid, and solid phases coexist is called triple point. The temperature and pressure in the phase diagram at which substance is lies between liquid-gas phases is called critical point. The temperature and pressure at which liquid or gas is neither a true liquid nor a true gas is called supercritical point.
Conversion of liquid into gas is called vaporization. Conversion of solid into liquid or vice-versa is called melting or fusion. Conversion of solid into gas is called sublimation.
Want to see the full answer?
Check out a sample textbook solutionChapter 11 Solutions
CHEMISTRY-W/MASTERING CHEMISTRY ACCESS
- 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_forwardDefine the joule in terms of SI base units.arrow_forwardCalculate the heat change in joules for freezing 235 gg of water at 0 ∘C∘C.arrow_forward
- Given that a 10.0g sample of ice at 0.0 degrees celsius melts and then the resultant water proceeds to warm to 20.0 degrees celsius, there are two separate processes (dealing with the transfer of heat) that describe the occurence. What are those two processes? (Hint one involves the specific heat of water). Determine the delta H of the following reactions: CH4 (g) +2O2(g) → CO2 (g) +2H2O(l) CH4 (g) +2O2(g) → CO2 (g) +2H2O(g) What is the numerical difference between these two values? What is the only physical difference between the two reactions? What does the numerical difference represent, in terms of the physical difference between the two reactions? A 4.00g sample of rocket fuel was combusted in a bomb calorimeter according to the following reaction: 2CH6N2(l)+ 5O2(g) → 2N2(g) +2CO2(g) + 6H2O(l) The temperature of the surrounding calorimeter increased from 25.00C to 39.50 C and the heat capacity of the calorimeter was previously determined to be 7.794KJ/c. What is the…arrow_forwardSulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73.0°C and boils at −10.0°C. Its ΔHfus is 8.619 kJ/mol, and its ΔHvap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g·K and 0.622 J/g·K, respectively. How much heat is required to convert 5.000 kg of solid SO2 at the melting point to a gas at 60.0 degrees C? Answer should be in J.arrow_forwardHow long (in seconds) would it take a 50.0 watt (1 watt = 1 J/s) heater to melt 10.02 g of Au(s) initially at its freezing point (1064 °C) to the boiling point (2807 °C) and then to completely vaporize it?arrow_forward
- The vapor pressure of benzene is 224 mmHg at 45 °C and 648 mmHg at 75 °C.(a) Find the enthalpy of vaporization of benzene, ∆Hvap (kJ/mol), assuming it is constant. You may also assume that ZV − ZL ≃ 1. B)arrow_forwardA 22.5-g sample of ice at 0.0°C is added to 100.0 g of warm water at 35.0°C, and the final temperature of the mixture is 14.0°C. (a) How much heat (in Joules) is lost by the warm water? (b) How much heat (in Joules) is absorbed by the melted ice when its temperature increases from 0.0°C to 14.0°C? (c) How much heat is absorbed by ice during melting at 0.0°C? (d) What is the enthalpy of fusion of ice in kJ/mol? 3. (Specific heat of water = 4.184 J/(g.°C)arrow_forwardWhat mass of steam initially at 130 °C is needed to warm 200. g of water in a 100. g glass container from 20.0 °C to 50.0 °C? The heat of vaporization of water is 2260 J g–1 . The specific heat of steam is 2.010 J g–1 °Carrow_forward
- How much energy is given off when 563.8 g of NaCl solidifies at its freezing point of 801C ?arrow_forward7. a) How much heat (in kJ) must be removed when cooling 155 g of benzene, C6H6, at 120.0°C to solid benzene at 5.48°C? Given for benzene: boiling point at 1 atm = 80.1 °C Melting point at 1 atm = 5.48°C Specific heat (I) = 1.74 J/ g x °C Specific heat (g) = 1.04 J/ g × °C Heat of fusion = 127 J/g Heat of vaporization = 395 J/g %3D %3D b) Nickel has a face-centered cubic unit cell. The density of nickel is 6.84 g/cm3. Calculate a value for the atomic radius of nickelarrow_forward(c) Is methane a solid, liquid, or gas at 1 atm and 0 °C? (d) If solid methane at 1 atm is heated while the pressure is held constant, will it melt or sublime? (e) If methane at 1 atm and 0 °C is compressed until a phase change occurs, in which state is the methane when the compression is complete?arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning