Calculate the lattice enthalpy(nearestinteger value) in kJmol-1 of LiF, given that,enthalpy ofsublimation of lithium is 155.3kJ mol-1 (i);dissociation of 1/2 mole of F2 is 75.3kJ (ii);ionization enthalpy of lithium is 520kJ mol-1 (iii)electron gain enthalpy of 1 mole of F(g) is -333k (iv)AfH overall is -594kJ mol-1 (v)

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Answered: Calculate the lattice enthalpy(nearest…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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O Discuss the factors affecting the sign of AG in the relationship AG= AH - TAS. Give examples for each of the situations,
Given the following reactions and their enthalpies: AH(kJ/mol) H;(g) 2H(g) 20(g) +436 O:(g) +495 H,(g) + 0,(g) → H,O(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.
Calculate the standard enthalpy of formation of NaHCO3(s) given the following information:rxn 1 1 NaOH(s) + CO2(g) ⟶ NaHCO3(s) ΔrH (rxn1) = −127.5 kJ mol-1ΔfH°[ CO2(g) ] = −393.41 kJ mol-1ΔfH°[NaOH(s) ] = −425.61 kJ mol-1
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.
Given the following data, calculate the lattice energy of barium chloride, BaCl. IE= 502.7 kJ mol IE = 965.0 kJ mol AHub (Ba) =175.6 kJ moľ" EA = 349.0 kJ mol" BDE (CI - CI) = 243.4 kJ mol AH(BaCl) = -858.6 kJ mol
Find the enthalpy of reaction for the equation: H2SO4laq) + 2NAOH(aq)-Na,SO,(aq) + 2H20(), AH=? Using the following equations whose enthalpy is known (please round your answer to the tenths place): H2(g) + S(s) + 202(g) – H2SO,(aq), AH= -907.5 kJ Na(s)+ ½H2(g) + ½O2{g) – NaOH(aq), AH= -469.6 kJ 2Na(s) + S(s) + 20,(g) – Na,SOal(aq). AH= -1387.1 kJ H2(8) + ½O2(g) – H2O(1). AH= -285.8 kJ AH= kJ.
AfH (298 K) = -859 kJ mol-¹, calculate a value for the lattice energy of BaCl₂. Outline any assumptions that you have made.
(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.
28. Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HC1O,(g), and c) CH;OCH;(g)
Use grade 12 chem knowledge to do this

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