Concept explainers
Interpretation:
To calculate the average
Concept introduction:
The
The change of enthalpy to form one mole of a substance from its constituent elements when all the substances in the standard form is known as standard enthalpy of formation.
The standard enthalpy of formation
Trending nowThis is a popular solution!
Chapter 21 Solutions
Chemistry & Chemical Reactivity
- The standard enthalpy of formation of XeF4 is 218 kJ/mol. Use this value and the enthalpy of dissociation of the FF bond to calculate the XeF bond dissociation enthalpy.arrow_forwardUsing the standard enthalpy of formation data, determine which bond is stronger: the P–Cl bond in PCl3(g) or in PCl5(g)?arrow_forwardA nonmetal like oxygen forms both ionic and covalent bonds, depending on the identity of the element to which it bonds. What type of bonding is observed in CaO and CO 2? Explain why two different types of bonding are observed.arrow_forward
- Answer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.arrow_forwardCalculate the lattice energy of AgBr(s) using the following thermodynamic data (all data is in kJ/mol). Ag(s) ΔHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Br-Br(g) Bond energy = 173 kJ/mol Br(g) Electron affinity = -345 kJ/mol AgBr(s) ΔH°f = -120 kJ/mol ______________ kJ/molarrow_forwardCalculate the standard enthalpy of formation of the M2O(s) metal oxide (AH+ in kJ/mol) using the following data: Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M + 116 kJ/mol First ionization energy of M = + 463 kJ/mol Lattice enthalpy of M₂O(s) = -2248 kJ/mol Refer to sections 9.4 and 9.5 in the textbook for definitions of ionization energy and electron affinity. Do not use scientific notation for your answer. Do not enter units. Your Answer:arrow_forward
- Use heat of formation data from Appendix E to calculate ∆H ° for the following reaction:ClO2 (g) + O(g) → ClO(g) + O2(g)arrow_forwardAnswer the questions in the table below about the shape of the borane (BH3) molecule. How many electron groups are around the central boron atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central boron atom? (You may need to use the scrollbar to see all the choices.) (choose one) X G <arrow_forwardConsider the reaction 2 S(g) + 3 O2(g) → 2 SO3(g). Using the standard enthalpies of formation listed in Appendix G of your text and the bond energy of 498.4 kJ/mol in molecular oxygen, calculate the average sulfur-oxygen bond energy, in units of kJ/mol, in sulfur trioxide gas. The answer is not 380/381.arrow_forward
- Use the above bond energy table to calculate the enthalpy of the following reaction in kJ/mol: 2H2CO2→ CO21E) + CHAE)arrow_forwardUsing the standard enthalpy of formation data , calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardWhy is ammonia a covalent bond?arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning