Concept explainers
Determine the lattice energy of KF(s) from the following data:
Learn your wayIncludes step-by-step video
Chapter 12 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Additional Science Textbook Solutions
Chemistry: The Central Science (14th Edition)
Chemistry: A Molecular Approach (4th Edition)
Chemistry (7th Edition)
Chemistry & Chemical Reactivity
Organic Chemistry
Introductory Chemistry (5th Edition) (Standalone Book)
- 9.46 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_forwardDefine the joule in terms of SI base units.arrow_forwardUse a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.arrow_forward
- How many KJ of heat are needed to raise the temperature of 10.0 Kg o fliquid water from 24.6 to 46.2oC?arrow_forwardA generic solid, X, has a molar mass of 65.9 g/mol. In a constant‑pressure calorimeter, 20.5 g of X is dissolved in 303 g of water at 23.00 °C. X(s)⟶X(aq) The temperature of the resulting solution rises to 29.30 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? What is the enthalpy of the reaction?arrow_forwardHow much energy (at constant temperature and pressure) must be supplied as heat to 10.0 g of chlorine gas (as Cl2) to produce a plasma (a gas of charged particles, in this case ions) composed of Cl− and Cl+ ions? The enthalpy of ionization of Cl(g) is +1257.5 kJ mol−1 and its electron-gain enthalpy is −354.8 kJ mol−1. ________ kJ. 4 sig. number.arrow_forward
- A 0.562 g sample of KCl is added to 35.8 g of water in a calorimeter. If the temperature decreases by 1.17°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?arrow_forward) The salt potassium perchlorate is soluble in water. When 2.84 g of KClO4 is dissolved in 106.00 g of water, the temperature of the solution decreases from 25.00 to 22.54 °C. Based on this observation, calculate the enthalpy of dissolution of KClO4 (in kJ/mol).Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.arrow_forwardWhat is the change in enthalpy when 38.2 g of CH4(g) reacts completly with O2(g) to form CH3OH(g) at constant pressure?arrow_forward
- A 5.00 g-sample of KOH at 25.0 C was added to 100.0 g of H2O(l) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH is a thermodynamically favorable process? A. The forces between the ions and the water molecules are stronger than the forces between water molecules, thus, delta H < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus delta S > 0. Therefore, delta G < 0. B. The energy require to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus delta H < 0. Also, the ions become widely dispersed as KOH(s) dissolved, thus delta S > 0. Therefore, delta G < 0. C. The average kinetic energy of the particles increases, resulting in delta H > 0. Also, the…arrow_forwardYou have substance X which is very flammable and substance Y which is very combustible in your garage in containers right in front of where you park your car. It is a hot July afternoon, 119Fand you just come home from work where your car was parked outside in the sun for 8 hrs and you were running the air conditioning the entire way home (hence, the car is very hot and is giving off a lot of heat). Which substance would you be more worried about and why ?arrow_forwardwhat quantity of heat would be evolved if 5.68g of liquid aluminum freezes at its normal freezing point?arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning