General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 12, Problem 25E
How many liters of
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 12 - For each of the following substances describe the...Ch. 12 - When another atom or group of atoms is substituted...Ch. 12 - Prob. 3ECh. 12 - Arrange the liquids represented by the following...Ch. 12 - One of the following substances is a liquid at...Ch. 12 - In which of the following compound might...Ch. 12 - Prob. 7ECh. 12 - Prob. 8ECh. 12 - Prob. 9ECh. 12 - Prob. 10E
Ch. 12 - Silicone oils, such as H3C[SiO(CH2)2],Si(CH3) ,...Ch. 12 - Surface tension, viscosity, and vapor pressure are...Ch. 12 - Is there any scientific basis for the colloquial...Ch. 12 - A television commercial claims that a product...Ch. 12 - Prob. 15ECh. 12 - Prob. 16ECh. 12 - Prob. 17ECh. 12 - Carbon tetrachloride (CCl4) and mercury have...Ch. 12 - As a liquid evaporated from an open container, its...Ch. 12 - Prob. 20ECh. 12 - The enthalpy of vaporization of benzene, C6H6(l)...Ch. 12 - A vapor volume of 1.17 L forms when a sample of...Ch. 12 - Use data from the Integrative Example (page 566)...Ch. 12 - How much heat is required to raise the temperature...Ch. 12 - How many liters of CH4(g) , measured at 23.4 °C...Ch. 12 - A 50.0 g piece of iron at 152°C is dropped into...Ch. 12 - From Figure 12-18, estimate (a) the vapor pressure...Ch. 12 - Prob. 28ECh. 12 - Equilibrium is established between Br2(l) and...Ch. 12 - Prob. 30ECh. 12 - A double boiler is used when a careful control of...Ch. 12 - One popular demonstration in chemistry labs is...Ch. 12 - Pressure cookers achieve a high cooking...Ch. 12 - Prob. 34ECh. 12 - A 25.0 L volume of He(g) at 30.0°C is passed...Ch. 12 - A 7.53 L sample of N2 (g) at 742 mmHg and 45.0 °C...Ch. 12 - Prob. 37ECh. 12 - A 10.0 g sample of liquid water is sealed in a...Ch. 12 - Cyclohexanol has a vapor pressure of 10.0 mmHg at...Ch. 12 - Prob. 40ECh. 12 - Prob. 41ECh. 12 - Prob. 42ECh. 12 - Benzaldehyde, C2H2CHO , has a normal boiling point...Ch. 12 - With reference to Figure 12-20, which is the more...Ch. 12 - Which substances listed in Table 12.6 can exist as...Ch. 12 - Prob. 46ECh. 12 - The normal melting point of copper is 1357 K, and...Ch. 12 - An ice calorimeter measures quantities of heat by...Ch. 12 - An 80.0 g piece of dry ice, CO2 (s), is placed in...Ch. 12 - Sketch a plausible phase diagram for hydrazine...Ch. 12 - Shown here is a portion of the phase diagram for...Ch. 12 - Prob. 52ECh. 12 - Prob. 53ECh. 12 - Prob. 54ECh. 12 - Use appropriate phase diagrams data from Table...Ch. 12 - Prob. 56ECh. 12 - To an insulated container with 100.0 g H2O(l) at...Ch. 12 - A 54 cm2 ice cube at 25.0 °C is added to a...Ch. 12 - Prob. 59ECh. 12 - Prob. 60ECh. 12 - Prob. 61ECh. 12 - Prob. 62ECh. 12 - Silicon carbide, SiC, crystallizes in a form...Ch. 12 - Prob. 64ECh. 12 - Prob. 65ECh. 12 - Use Coulomb's law (see Appendix B) to verify the...Ch. 12 - The hardness of crystals is rated based on Mohs...Ch. 12 - Will the mineral villaumite (NaF) or periclase...Ch. 12 - Prob. 69ECh. 12 - Prob. 70ECh. 12 - Consider the two-dimensional lattice shown here....Ch. 12 - As we saw in Section 12-6, stacking spheres always...Ch. 12 - Tungsten has a body-centered cubic crystal...Ch. 12 - Magnesium crystallizes in the hcp arrangement...Ch. 12 - Polonium (Po) is the only element known to take on...Ch. 12 - Prob. 76ECh. 12 - Silicon tetrafluoride molecules are arranged in a...Ch. 12 - Two views, a top and side view, for the unit cell...Ch. 12 - Show that the unit cells for CaF2 and TiO2 in...Ch. 12 - Prob. 80ECh. 12 - The crystal structure of magnesium oxide, MgO, is...Ch. 12 - Potassium chloride has the same crystal structure...Ch. 12 - Prob. 83ECh. 12 - Use data from Figure 9-9 to predict the type of...Ch. 12 - Without doing calculations, indicate how you would...Ch. 12 - Determine the lattice energy of KF(s) from the...Ch. 12 - Refer to Example 12-12. Together with data given...Ch. 12 - Prob. 88ECh. 12 - Prob. 89IAECh. 12 - Prob. 90IAECh. 12 - Prob. 91IAECh. 12 - Use the following data and data from Appendix D to...Ch. 12 - Prob. 93IAECh. 12 - Prob. 94IAECh. 12 - Because solid p-dichlorobenzene, C6H4CI2 ,...Ch. 12 - A 1.05 mol sample of H2O(g) is compressed into a...Ch. 12 - Prob. 97IAECh. 12 - By the method used to graph Figure 12-20, plot In...Ch. 12 - Prob. 99IAECh. 12 - Prob. 100IAECh. 12 - Prob. 101IAECh. 12 - Prob. 102IAECh. 12 - In acetic acid vapor, some molecules exist as...Ch. 12 - Prob. 104IAECh. 12 - Sketched here are two hypothetical phase diagrams...Ch. 12 - Prob. 106IAECh. 12 - The triple point temperature of bismuth is 544.5 K...Ch. 12 - The crystal structure of lithium sulfide ( Li2S ),...Ch. 12 - Refer to Figure 12-44 and Figure 12-48. Suppose...Ch. 12 - Prob. 110IAECh. 12 - One way to describe ionic crystal structures is in...Ch. 12 - Prob. 112IAECh. 12 - The enthalpy of formation of Nal(s) is 288 kJ...Ch. 12 - Prob. 114IAECh. 12 - A crystalline solid contains three types of ions,...Ch. 12 - A certain mineral has a cubic unit cell with...Ch. 12 - Prob. 117IAECh. 12 - In some barbecue grills the electric lighter...Ch. 12 - Prob. 119IAECh. 12 - Prob. 120IAECh. 12 - Intermolecular forces play vital and varied roles...Ch. 12 - Prob. 122FPCh. 12 - Prob. 123FPCh. 12 - All solids contain defects or imperfections of...Ch. 12 - In an ionic crystal lattice each cation will be...Ch. 12 - Prob. 126FPCh. 12 - Prob. 127FPCh. 12 - Prob. 128SAECh. 12 - Briefly describe each of the following phenomena...Ch. 12 - Explain the important distinctions between each...Ch. 12 - Prob. 131SAECh. 12 - Prob. 132SAECh. 12 - Prob. 133SAECh. 12 - Prob. 134SAECh. 12 - Prob. 135SAECh. 12 - Prob. 136SAECh. 12 - Prob. 137SAECh. 12 - Prob. 138SAECh. 12 - Prob. 139SAECh. 12 - Prob. 140SAECh. 12 - Prob. 141SAECh. 12 - Prob. 142SAECh. 12 - Prob. 143SAECh. 12 - Prob. 144SAECh. 12 - The following data are given for CCl4 . Normal...Ch. 12 - The fcc unit cell is a cube with atoms at each of...Ch. 12 - Prob. 147SAECh. 12 - Prob. 148SAECh. 12 - Prob. 149SAECh. 12 - Prob. 150SAECh. 12 - In the lithium iodide crystal, the Li—l distance...Ch. 12 - Prob. 152SAECh. 12 - Prob. 153SAECh. 12 - Prob. 154SAECh. 12 - Construct a concept map showing the ideas...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- If 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_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_forwardThe cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.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_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_forwardA student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)arrow_forward
- Suppose you wanted to cool 100. g of water from 20 C to 0 C using dry ice, CO2(s). The enthalpy of sublimation of CO2(s) is 25.2 kJ/mol. What mass of dry ice should you need? (a) 033 g (b) 15 g (c) 3.5 g (d) 150 garrow_forwardAre 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_forward
- The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)arrow_forwardAn industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?arrow_forwardThe enthalpy of combustion of liquid n-hexane, C6H14, is 4159.5 kJ/mol, and that of gaseous n-hexane is 4191.1 kJ/mol. Use Hesss law to determine H for the vaporization of 1 mol of n-hexane: C6H14() C6H14(g)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningPhysical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth 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
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY