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Consider the following
C3H8(g) + 5 O2(g) → 3 CO2(g) +4 H2O(g)
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- Bond Energies (kJ/mol) Bond Bond Energy Bond Bond Energy Bond Bond Energy H–H 436 C–S 260 F–Cl 255 H–C 415 C–Cl 330 F–Br 235 H–N 390 C–Br 275 Si–Si 230 H–O 464 C–I 240 Si–P 215 H–F 569 N–N 160 Si–S 225 H–Si 395 N=NN=N 418 Si–Cl 359 H–P 320 N≡NN≡N 946 Si–Br 290 H–S 340 N–O 200 Si–I 215 H–Cl 432 N–F 270 P–P 215 H–Br 370 N–P 210 P–S 230 H–I 295 N–Cl 200 P–Cl 330 C–C 345 N–Br 245 P–Br 270 C=CC=C 611 O–O 140 P–I 215 C≡CC≡C 837 O=OO=O 498 S–S 215 C–N 290 O–F 160 S–Cl 250 C=NC=N 615 O–Si 370 S–Br 215 C≡NC≡N 891 O–P 350 Cl–Cl 243 C–O 350 O–Cl 205 Cl–Br 220 C=OC=O 741 O–I 200 Cl–I 210 C≡OC≡O 1080 F–F 160 Br–Br 190 C–F 439 F–Si 540 Br–I 180 C–Si 360 F–P 489 I–I 150 C–P 265 F–S 285 Molecular ekacagine combines with ethylene to form diekaethylene (C2H2Ec2) according to the reaction below: Examine the bond energies in Table 9.3 of your textbook. Shuri’s undergrads measured the new bond enthalpies: C-Ec bond energy is 220 kJ/mol and the…Given the following thermodynamic data, calculate the lattice energy of LiCl:ΔH°f[LiCl(s)] = -409 kJ/molΔH°sublimation [Li] = 161 kJ/molBond energy [Cl-Cl] = 243 kJ/molIE1 (Li) = 520 kJ/molEA1 (Cl) = -349 kJ/mol -1682 kJ/mol -984 kJ/mol -1560 kJ/mol -862 kJ/mol -1213 kJ/molUse the bond energies provided to estimate ΔH°rxn for the reaction below.XeF2 + 2 F2 → XeF6ΔH°rxn = ? Bond Bond Energy (kJ/mol) Xe-F 147 F-F 159
- Some of bond energies (kJ/mol)H-H: 436C-H: 416C-C single bond: 356C-C double bond: 598C-C triple bond: 813N-H: 391C-N: 285N-N: 160N-N triple bond: 946O-H: 467C-O single bond: 336C-O double bond: 803N-O: 201O-O double bond: 498Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891 Cl-Cl 243 S-Cl 250 S=O 535 S-S 215 S-O 364 S-H 339 Using the table of bond energies above, estimate the enthalpy change (kJ) for the following reaction: CH4+2O2⟶CO2+2H2OThe Bond energy of C2(g) is 599 kJ/mol and for F2 is 154 kJ/mol. Use MO theory to justify the difference.
- Use the table below to determine ΔH for the following reactionN 2H 4(g) + H 2O(g) ↔ NH 2OH(g) + NH 3(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 C≡C 835 C≡N 887 C≡O 1072 N=N 418 N=O 607 S=O (in SO2) 532 N≡N 942 O2 494 S=O (in SO3) 469Which of the following electron configuration pairs would most likely result in covalent bonding? A. 1s2 2s2 2p5 and 1s2 2s2 2p6 B. 1s2 2s2 2p5 and 1s2 2s2 2p5 C. 1s2 2s2 and [Ar] 4s1 D. [Ne] 3s1 and [Ne] 3s1Consider the following reaction:H2 (g) + O2 (g) --> H2O2 (g) (Delta)H = -153 kJGiven that the H2 bond energy is 432 kJ/mol, the O2 bond energy is 495 kJ/mol, and the OH bond energy is 467 kJ/mol, estimate the bond energy for the oxygen-oxygen single bond (in kJ/mol).
- Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 458.5 kJ/molΔHof of X2O4(g) is 31 kJ/molThe X-X single bond energy is 116 kJ/molUse the above data to estimate the average bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.2.7 Which of the following electron configurations belongs to an atom that is most likely to be involved in an ionic bond? 1s22s22p63s2 1s22s22p63s23p6 1s22s22p6 1s22s22p63s23p3Is this correct? (I think the degree symbol represents a triple bond)