E15C.5(a) Calculate the lattice enthalpy of CaO from the following data:AH/(kJ mol")Sublimation of Ca(s)+178Ionization of Ca(g) to Ca³"(g)Dissociation of O,(g)+1735+249Electron attachment to O(g)Electron attachment to O (g)Formation of CaO(s) from Ca(s) and }0,(g)in their reference states.-141+844-635

Lattice enthalpy : The energy released when the ions combines, because of strong electrostatic…

Answered: E15C.5(a) Calculate the lattice…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 35QRT

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C(s, graphite) + H,O(g) → CO(g) + H, (g) ASixn J/mol·K 2 H,0,(1) 2 H,0(0) + О,(g) J/mol·K rxn
E15C.5(b) Calculate the lattice enthalpy of MgBr, from the following data: AH/(kJ mol") Sublimation of Mg(s) +148 Ionization of Mg(g) to Mg*(g) +2187 Vaporization of Br,(1) Dissociation of Br,(g) Electron attachment to Br(g) Formation of MgBr,(s) from Mg(s) and Br,(1) in their reference states. +31 +193 -331 -524
The 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.
Given 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.
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
Hydrazine, N3H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N3(9) + 2H2 (9) + N2H4 (1) Use the following reactions and enthalpy changes: N2H, (1) + O2 (9) + N2(9) + 2H, 0(1); AH = -622.2 kJ H2 (9) +O2(g) H20(1); AH = -285.8 kJ ΔΗ- k)
Two positively charged spheres, each with a charge of 2.0x 10-5 C, a mass of 1.0 kg, and separated by a distance of 1.0 cm, are held in place on a frictionless track. (a) What is the electrostatic potential energy of this system? (b) If the spheres are released, will they move toward or away from each other? (c) What speed will each sphere attain as the distance between the spheres approaches infinity?
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)
(a) What is the electrostatic potential energy (in joules) betweentwo protons that are separated by 62 pm? (b) Whatis the change in potential energy if the distance separatingthe two is increased to 1.0 nm? (c) Does the potential energyof the two particles increase or decrease when the distanceis increased to 1.0 nm?
(d) Which salt, LiCl or NaCl, has the greater lattice enthalpy? Justify your answer. (e) Below is a representation of a portion of a crystal of LiCl. Identify the ions in the representation by writing the appropriate formulas (Li* or CT) in the boxes below.
Alkali metals are often used to remove traces of water from organic solvents, such as diethyl ether. Because the reaction (see below) releases heat, care must be taken to make sure that the solvent does not "boil over". 2 Na(s) + 2 H₂O(1) ➜ 2 NaOH(aq) + H₂(g) a) Determine the standard enthalpy change for this reaction. Comment on the relative strength of bonding and/or interactions in the products vs reactants, and briefly explain how you decided this. Substance Na(s) H₂O(1) NaOH(aq) H₂(g) AHºf (kJ/mol) 0 -285.83 -469.15 0 b) How much heat (in kJ) is released via the reaction of 1.00 g of sodium metal with water? If this much heat is released into 275 g of diethyl ether initially at 25°C, will the solvent reach its boiling point? If so, how many grams of the ether will evaporate? Show calculations to support your answer. For diethyl ether: Cs = 2.51 J/g⋅K, b.p. = 35°C, heat of vaporization = 377 J/g.
(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 kJ

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