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We saw in Section 6.7 that the reaction of solid sodium with giseous chlorine to yield solid sodium chloride
Assume that the lattice energy for
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LCPO CHEMISTRY W/MODIFIED MASTERING
- Bromine-containing species play a role in environmental chemistry. For example, they are evolved in volcanic eruptions. (a) The following molecules are important in bromine environmental chemistry: HBr, BrO, and HOBr. Which is an odd-electron molecule? (b) Use bond dissociation enthalpies to estimate rH for three reactions of bromine: Br2(g) 2 Br(g) 2 Br(g) + O2(g) 2 BrO(g) BrO(g) + H2O(g) HOBr(g) + OH(g) (c) Using bond dissociation enthalpies, estimate the standard enthalpy of formation of HOBr(g) from H2(g), O2(g), and Br2(g). (d) Are the reactions in parts (b) and (c) exothermic or endothermic?arrow_forwardThe equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol? (b) Compare your answer in part (a) with the value of tHcalculated using enthalpies of formation data.arrow_forwardCalculate the lattice energy of potassium fluoride, KF, using the BornHaber cycle. Use thermodynamic data from Appendix C to obtain the enthalpy changes for each step. (Note: You will obtain a slightly different answer if you use values given in Chapter 8 for the ionization energy and electron affinity, which are energy values at 0 K rather than the enthalpy changes at 298 K.)arrow_forward
- Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardConsider the reactions of silver metal, Ag(s), with each of the halogens: fluorine, F2(g), chlorine, Cl2(g), and bromine, Br2(l). What chapter data could you use to decide which reaction is most exothermic? Which reaction is that?arrow_forwardThe standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are + 278.8, + 79.0, 775, and 1209 kJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 8.5. What conclusions can you draw? c. Why are the Ht0 values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forward
- Which compound in each of the following pairs of ionic substances has the most negative lattice energy? Justify your answers. a. LiF, CsF b. NaBr, NaI c. BaCl2, BaO d. Na2SO4, CaSO4 e. KF, K2O f. Li2O, Na2Sarrow_forwardThe lattice energy of NaBr is –752 kJ/mol. This energy corresponds to which reaction below? Na(s) + 1/2 Br2(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na+(g) + Br–(g) → NaBr(s) Na+(aq) + Br–(aq) → NaBr(s)arrow_forwardChoose the related energy for the following reaction: 2 Cs* (g) + O2- (g) → Cs20 (s) electron affinity ionization energy heat of formation lattice energyarrow_forward
- The enthalpy change for the reaction between two molecules of carbon oxysulfide (COS) to form one molecule of CO2 and one molecule of CS2, as shown below, is –3.2 × 10–24 kJ per molecule of COS. The bond energy for the C=S bond in CS2 has been determined to be 552 kJ/mol. What is the apparent bond energy of a carbon–sulfur bond in COS? Use the bond energies below. Bonds Bond Energy(kJ/mole) C=S 552 C=O 799 Note: A C=O bond adjacent to another double bond is not the same as a C=O bond that is not adjacent to another double bond.arrow_forwardThe energy for the following reaction was measured to be -1033.0 kJ/mol. Mg(g) + 2 Cl(g) → MgCl,(s). Using this fact and the data in the table below, calculate the enthalpy (in kJ/mol) required to separate the ions from the lattice for this reaction: MgCl₂(s) → Mg²+(g) + 2Cl(g). Substance Ionization Energies (kJ/mol) Electron (kJ/mol) 0 Mg (g) 737.8 Mg* (g) 1450.7 CI (g) 1251.2 -349arrow_forward5. Consider the following information: 1st ionization energy of Na(g) = 495.8 kJ/mol Bond dissociation energy of O2(g) = 498.4 kJ/mol 1st electron affinity of O(g)=-142.5 kJ/mol 2nd electron affinity of O¹(g) = 844 kJ/mol Lattice energy of Na2O(s) = -2608 kJ/mol Enthalpy of formation of Na2O(s) = -416 kJ/mol a Draw the Born-Haber cycle for Na₂O(s). b Calculate the unknown. 120 C Draw the Lewis symbol for Na₂O.arrow_forward
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