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(a)
Interpretation:
The specific
Concept introduction:
The amount of energy released when one formula unit moles of oppositely charged gaseous ions binds together to form a crystal is known as the lattice energy. The value of lattice energy is negative. It is used as a measure for stability of a crystal.
(b)
Interpretation:
The specific chemical reaction whose enthalpy change represents the lattice energy of the given solid is to be stated.
Concept introduction:
The amount of energy released when one formula unit moles of oppositely charged gaseous ions binds together to form a crystal is known as the Lattice energy. The value of lattice energy is negative. It is used as a measure for stability of a crystal.
(c)
Interpretation:
The specific chemical reaction whose enthalpy change represents the lattice energy of the given solid is to be stated.
Concept introduction:
The amount of energy released when one formula unit moles of oppositely charged gaseous ions binds together to form a crystal is known as the Lattice energy. The value of lattice energy is negative. It is used as a measure for stability of a crystal.
(d)
Interpretation:
The specific chemical reaction whose enthalpy change represents the lattice energy of the given solid is to be stated.
Concept introduction:
The amount of energy released when one formula unit moles of oppositely charged gaseous ions binds together to form a crystal is known as the Lattice energy. The value of lattice energy is negative. It is used as a measure for stability of a crystal.
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Chapter 21 Solutions
EBK PHYSICAL CHEMISTRY
- The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?arrow_forwardUsing a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.arrow_forwardHydrogen, H2, is prepared by steam reforming, in which hydrocarbons are reacted with steam. For CH4, CH4(g)+H2O(g)CO(g)+3H2(g) Calculate the enthalpy change H for this reaction, using standard enthalpies of formation.arrow_forward
- When boron hydrides burn in air, the reactions are very exothermic (a) Write a balanced equation for the combustion of B5H9(g) in air to give B2O3(s) and H2O(g). (b) Calculate the enthalpy of combustion for B5H9(g) (fH = 73.2 kJ/mol), and compare it with the enthalpy of combustion of B2H6 (2038 kJ/mol). (The enthalpy of formation of B2O3(s) is 1271.9 kJ/mol.) (c) Compare the enthalpy of combustion of C2H6(g) with that of B2H6(g). Which transfers more energy as heat per gram?arrow_forward(b) What is the first law of thermodynamic? Define the Hess law. Given the following data; 2CIF(g) + 0,(g) CI,0(g) + F,O(g) AH = 167.4 kJ AH = 341.4 kJ SH = -43,4 kJ 2CIF,(g) + 20,(g) → CĻ0(g) + 3F,O(g) 2F,(2) + O(8) → 2F,O(g) calculate AH for the reaction CIF(g) + F(8) CIF,(g)arrow_forward(ii) The industrial process for producing sulphuric acid, H2SO4, from elemental sulphur has three steps, using the information below; (a) identify the three steps, and describe the nature of each step (in one phrase); (b) write an equation for the overall reaction. (c) using the data given below, calculate the enthalpy change for the overall reaction. S(s) + O2(g) SO-(g) A;H° = -296.8 kJ 2S0:(g) 2SO2(g) + O2(9) A;H° = -198.2 kJ SO((g) + H2O(1) H2SO4() A;H° = -227.7 kJarrow_forward
- The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of formation in Appendix C to estimate the enthalpy of this bond, D(N‚N).arrow_forwardGiven the following ræactions and their enthalpies: ΔΗ (k/mol), +436 2H(g) H2(g) 0,(g) - 20(g) +495 H(g) + 02(g) Н.О(g) -242 (a) Devise a way to calculate AH for the reaction H,O(g) → 2H(g) + O(g) (b) From this, estimate the H-O bond energy.arrow_forwardWhat is the electrostatic potential energy between an electron and a proton that are separated by 53 pm?arrow_forward
- Which reaction is the formation reaction for CaO(s)? In other words, which equation has a AHn value equal to the AH; value for CaO(s) Ca?+(aq) + O2-(aq) · CaO(s) Ca(s) + 0,(g) — СаО(s) O 2 Ca(s) + O,(g) — 2 СаО(s) O 2 CaO(s) 2 Ca(s) + O2(g) > О Са0(s) — Сa('s) + 30,(g)arrow_forward(a) Consider the hypothetical element X. XO reacts with hydrogen gas to form XH;OH. Calculate the enthalpy of this reaction given that: (i) the enthalpy change that occurs when X reacts with oxygen gas to form XO is -221.0 kJ (ii) the enthalpy change that occurs when X reacts with oxygen gas and hydrogen gas to form XH,OH is -402.4 kJ. Calculate the distance between the centers of Y²* and Z² ions in a YZ lattice given that when 3.6 g of the compound are formed from its gaseous ions, 3.8 kJ of energy are released. The proportionality constant, k = 8.01 x 101" J pm. Molar mass of YZ: 257 g moľ' (b) (c) When a sample of vanadium metal absorbs 353 kJ of energy, the 'd' electrons of the metal atoms undergo a transition from their ground state to the fifth electron shell. Calculate the mass of this metal sample.arrow_forwardThe enthalpy changes accompanying the dissociation of successive bonds in NH3(g) are 460, 390, and 314 kJ mol-1 , respectively. (a) What is the mean enthalpy of an N-H bond? (b) Do you expect the mean bond internal energy to be larger or smaller than the mean bond enthalpy? (c) Use these values,along with tabulated bond enthalpies for the N-N and H-H bonds to estimate the standard enthalpy of formation of gaseous ammonia, NH3 , at 298 K.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningWorld of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College DivChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral 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
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