51) Use the bond energies provided to estimate ΔH°rxn for the reaction below. 2 Br2(l) + C2H2(g) → C2H2Br4(l)ΔH°rxn = ? BondBond Energy (kJ/mol) Br-Br193 C≡C837 C-C347 C-Br276 C-H414 A) +407 kJ B) -324 kJ C) -228 kJ D) +573 kJ E) -648 kJ 52) Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g)ΔH°rxn = ? BondBond Energy (kJ/mol) C-H414 C-O360 C=O799 O=O 498 O-H464 A) +473 kJ B) -91 kJ C) -486 kJ D) -392 kJ E) +206 kJ 53) Use the bond energies provided to estimate ΔH°rxn for the reaction below. XeF2 + 2 F2 → XeF6ΔH°rxn = ? BondBond Energy (kJ/mol) Xe-F147 F-F159 A) -429 kJ B) +159 kJ C) -660 kJ D) +176 kJ E) -270 kJ 54) Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g)ΔH°rxn = -197.8 kJ A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ 55) Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction 4 SO3(g) → 4 S(s) + 6 O2(g) ΔH°rxn = ? Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2 SO3(g)ΔH°rxn = -197.8 kJ A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ 56) Which of the following is not a standard state? A) For a solid, it is 25°F. B) For a liquid, it is 25°C. C) For a gas, it is 1 atm. D) For a solution, it is 1 M. E) For a liquid, it is 1 atm. 57) Which of the following is not a standard state? A) For a liquid, it is 25°F. B) For a solid, it is 25°C. C) For a solid, it is 1 atm. D) For a solution, it is 1 M. E) For a liquid, it is 1 atm. 58) Choose the thermochemical equation that illustrates ΔH°f for Li2SO4. A) 2 Li+(aq) + SO42-(aq) → Li2SO4(aq) B) 2 Li(s) + 1/8 S8(s, rhombic) + 2 O2(g) → Li2SO4(s) C) Li2SO4(aq) → 2 Li+(aq) + SO42-(aq) D) 8 Li2SO4(s) → 16 Li(s) + S8(s, rhombic) + 16 O2(g) E) 16 Li(s) + S8(s, rhombic) + 16 O2(g) → 8 Li2SO4(s) 59) Use the ΔH°f information provided to calculate ΔH°rxn for the following  ΔH°f (kJ/mol) SO2Cl2(g) + 2 H2O(l) → 2 HCl(g) + H2SO4(l)ΔH°rxn = ? SO2Cl2(g)-364 H2O(l)-286 HCl(g)-92 H2SO4(l)-814 A) -256 kJ B) +161 kJ C) -62 kJ D) +800. kJ E) -422 kJ 60) Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF  ΔH°f (kJ/mol) IF7(g) + I2(g) → IF
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