Identify the correct dipole for the C-O bond in the Lewis structure of acetone shown using the symbols δ⁺ and δ⁻.   A (δ⁺)C – O(δ⁺) B (δ⁻)C – O(δ⁺) C (δ⁻)C – O(δ⁻) D (δ⁺)C – O(δ⁻)

Use bond enthalpies in Table 5.4 to estimate ΔH for each ofthe following reactions:

Find ΔH for CO2 (g) + H2 (g) →    CO (g) + H2O (g)  given     C3H8 (g) + 3 H2O (g) → 3 CO (g) + 7 H2 (g)   ΔH = 499 kJ                C3H8 (g) + 6 H2O (g) → 3 CO2 (g) + 10 H2 (g) ΔH = 364 kJ

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)   3 C(s) + 4 H2(g) → C3H8(g)           ΔH = – 118.2 kJ C(s) + O2(g) → CO2(g)                   ΔH = – 62.4 kJ H2(g) + 1/2 O2(g) →  H2O(g)          ΔH = – 182.5 kJ

Calculate the ΔH  for the following reaction using the given bond energies.  (H - C = 414; C - C = 347; C = C = 619; H - H = 435). CH2 = CH2(g) + H2(g) => CH3 - CH3(g)

Use bond enthalpies in Table 5.4 to estimate ΔH for each ofthe following reactions:

Please answer question 13 part A

What is ΔHof of Al2S3(s)?   2Al2S3(s) + 9O2(g) → 2Al2O3(s) + 6SO2(g)     ΔHo = -3684.2 kJ   ΔHof  Al2O3(s) = -1675.7 kJ/mol  ΔHof  SO2(g) = -296.8 kJ/mol

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) 469

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N2H4(l) + 2 H2O2(g) → N2(g) + 4 H2O(l) N2H4(l) + O2(g) → N2(g) + 2 H2O(l)       ΔH = – 120.4 kJH2(g) + 1/2 O2(g) → H2O(l)                    ΔH = + 69.7 kJH2(g) + O2(g) → H2O2(l)                       ΔH = +54.8 kJ