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 a Born-Haber Cycle to calculate the missing ∆H (bold reaction) of the following:     Be(g) yields  Be2+(g) + 2 e–                                   ∆H= +2660 kJ/mole              Be(s)  yields  Be(g)                                                ∆H= +302 kJ/mole              1/2 I2(s)  yields  I(g)                                             ∆H= +107 kJ/mole             I(g) + e–   yields   I–(g)                                            ∆H= –295 kJ/mole            Be2+(g) + 2 I–(g) yields   BeI2(s)                        ∆H= ?                    Be(s) + I2(s) yields  BeI2(s)                      ∆H= –208 kJ/mole BeI2

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

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

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)

Find the AH for the reaction below, given the following reactions and subsequent AH values: B2H6(g) + 6 Cl2(g) → 2 BCI3(g) + 6 HCI(g) ΔΗ = – 72.5 kJ BC13(g) + 3 H₂O(l) → H3BO3(g) + 3 HCI(g) B2H6(g) + 6 H₂O(l) → 2 H3BO3(s) + 6 H2(g) ΔΗ = + 60.8 kJ 1/2 H₂(g) + 1/2 Cl₂(g) → HCI(g) 150.3 kJ ΔΗ = -

Which reaction below should have a positive value of AS? O2 NO2(g) → N₂O4(g) BaF2 (s) → Ba²+ (aq) + 2 F- (aq) 2 Hg(1) + O2(g) → 2 HgO (s) 2 H₂(g) + O2(g) → 2 H₂O(g) OH(aq) + F(aq) → HF (aq) Which of the following represents an oxidation-reduction reaction? all of these OC(s) + O2(g) → CO₂(g) two of these OH₂CO3 → 2 H+ + CO²- O CO2 + H₂O → H₂CO3

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

From the following data, calculate the average bond enthalpy for the N-H bond: NH3(g)NH2(g)+ H(g) AH = 435 kJ/mol NH2(g) NH(g) H(g) AH = 381 kJ/mol NH(g) N(g)H(g) AH = 3.60 x 102 kJ/mol kJ/mol

Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:   2 OF2(g) + 2 S(s) → SO2(g) + SF4(g)   OF2(g) + H2O(l) → O2(g) + 2 HF(g)             ΔH = – 78.5 kJSF4(g) + 2 H2O(l) →  4 HF(g) + SO2(g)          ΔH = + 62.7 kJS(s) + O2(g) → SO2(g)                     ΔH = – 154.3 kJ