Use the information provided to determine AH rxn for the following reaction CH4(9) + 3 Cl2(g) - CHC13(1) +3 HCI(g) AH°f (kJ/mol) CH4(9) -73 CHC13(1)-142 HCI(g) -95 AH*rxn=?
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- 5. Calculate AH xn for the combustion of butanol: CH3CH2CH2CH2OH (I) + 6 O2 (g)→4 CO2 (g) +5 H2O (g) Compound AH"r (kJ/mol) C4H9OH (I) -332.8 CO2 (g) -393.5 H20 (g) -241.8Given the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ Calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)16. Given the following set of reaction data, C(s) +O2(g) → CO2(8) AH = -393.5 kJ mol → 2CO2(8) 2H,0(g) AH = -566.0 kJ mol 2C0(g) + O2(g) 2H, (g) + O2(8) - AH = –483.6 kJ mol¬ determine the molar enthalpy (in kJ mol) for the following reaction. C(s) + H,O(g) – CO(g) + H2(g) AH = ? kJ mol-1 A: 1.31 x 102
- Calculate AHrxn for the reaction: 7 C(s) + 8 H2 (g)→ C,H16 (g) The following reactions and associated AHrxn values are may likely be helpful to you: C;H16(g) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (g) C (s) + O2 (g) → CO2 (g) 2 H2 (g) + O2 (g) → 2 H20 (g) Reaction A: AHrxn = -4817 kJ Reaction B: ΔΗn = -393.5 kJ Reaction C: AHrxn = -483.6 kJ (A) -128.1 kJ (B) 9509.9 kJ (C) 3939.9 kJ (D) 128.1 kJ (E) -9505.9 kJGiven the data below, H°, for the reaction rxn 2SO2 (g) + O2 (g) → 2SO3 (g) is kJ. AH°; (SO2 (g)) = -297 kJ/mol AH°; (SO3 (g)) = -396 kJ/mol AH°; (SO2C12 (g)) = -364 kJ/mol AH°f (H2SO2 (1)) = -814 kJ/mol AH°; (G2O (1)) = -286 kJ/mol %3D O The AH°F of O2 (g) is needed for the calculation. 99 198 -198 -99C+½ 020l co CO (s) 2 (g) CO+ 2 02(a) (g) AH = - 111 kJ %3D CO, 2 (g) Is this reaction endothermic or exothermic? (g) AH = - 394 kJ %3D -11 K3+(-394 C6st O2 (9)-yCO26) AH=-505 KJ Exothermic 2. a) Explain how AT would be affected if a greater amount of surrounding solvent (water) is used, assuming the mass of salt remains constant? b) Explain how qien would be affected if a greater amount of surrounding solvent (water) is used? Explain. If the following enthalpies are known: AH = - 95KJ 2 C+D A+2B- C) AH = + 50kJ B+X
- Given the following reaction: CH4G) + O2ig) + Cs) + 2H,00 ΔΗ - 118.7 kcal 1 Cs) + O2lg) → CO(g) AH° - 26.4 kcal 2 1 O2ig) → CO29) AH° = - 67.7 kcal 2 Consider the combustion of methane, determine the AH° using Hess's Law. CH49) + 202ig) → CO2(@) + 2H,O0 ΔΗ- =[4] rxn 2. Given the following information, calculate AH for the reaction. 2C3Hs(g) +1002(g) → 6CO2(g) + 8H₂O(1) | AH¦ (C³H8(g)) = -103.9 kJ/mol; AH; (CO2(g)) = -393.5 kJ/mol, AH; (H₂O(1) = -285.5 kJ/mol2SO2 (g) 02 (9) → 2SO3 (g) + (AHF° SO2 (g) = -296.8 kJ/mol; AHf ° SO3 (g) = -395.7 kJ/mol)
- Given the following data: C2H2(g) + 5/2 O2(g) --> 2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) + O2(g) --> CO2(g) ΔH= -394kJ H2(g) + 1/2O2(g) --> H2O(l) ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) --> C2H2(g)P4(s) + 5O2(g) → P4O10(s) ∆ G° = -2697.0 kJ/mol2H2(g) + O2(g) → 2h2O(g) ∆ G° = - 457.18 kJ/mol 6H2O(g) + P4O10(s) → 4H3PO4(1) ∆G° = - 428.66 kJ/mol What is the standard free energy of formation, ∆ Gf degree, for phosphoric acid? a: 11243.3 kj/mol b: -11243.3 kj/mol c: 4497.2 kj/mol d: -4497.2 kj/molWhat amount of energy is released (in the form of heat) when 60.0g of 1-pentanol reacts with oxygen? (Molar mass of 1-pentanol = 88.2g/mole) * 2CH3 (CH2)40H + 150u2) → 10COue) + 12H201e) A H° = -3330KJ