Using the table of average bond energies below, the AH for the reaction is kJ. C=O (g) + 2H2 (g) - НзC-0-Н (9) Bond: C-O C=O C-H H-H 0-Н D (kJ/mol). 358 799 1072 413 436 463
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- Isomers are molecules with the same elemental composition but a different atomic arrangement. Three isomers with the formula C4H8 are shown in the models below. The enthalpy of combustion (cH) of each isomer, determined using a calorimeter, is as follows: (a) Draw an energy level diagram relating the energy content of the three isomers to the energy content of the combustion products, CO2(g) and H2O(). (b) Use the cH data in part (a), along with the enthalpies of formation of CO2(g) and H2O() from Appendix L, to calculate the enthalpy of formation for each of the isomers. (c) Draw an energy level diagram that relates the enthalpies of formation of the three isomers to the energy of the elements in their standard states. (d) What is the enthalpy change for the conversion of cis-2-butene to trans-2-butene?Find the heat of reaction and explain what happen to it. Calculate the ∆H of reaction for: C3H8 (g) + 5O2 (g) => 3CO2 (g) + 4H2O (l) The values of ∆H of reaction are as follows:C3H8 (g) = -103.95 kJ/molCO2 (g) = -393.5 kJ/molH2O (g) = -285.8 kJ/mol Topic: Enthalpy of Reaction0 Calculate AH for the following reaction, after it is properly balanced with smallest whole-number coefficients: rxn C,H%(g) + Ozg) → COz(g) + H,O(g) AH [C₂H6(g)] = -84.667 kJ/mol AH [CO₂(g)] = -393.5 kJ/mol AH [CO₂(aq)] = −412.9 kJ/mol AH [H₂O(g)]=-241.826 kJ/mol AH [H₂O()] = -285.840 kJ/mol f kJ [unbalanced]
- Find ΔG°rxn for the reaction: N2O(g) + NO2(g)¡ 3 NO(g) Use the following reactions with known ΔG°rxn values:2 NO(g) + O2(g)¡2 NO2(g) ΔG°rxn = -71.2 kJN2(g) + O2(g)¡2 NO(g) ΔG°rxn = +175.2 kJ2 N2O(g)¡2 N2(g) + O2(g) ΔG°rxn = -207.4 kJDiethyl ether, C4H10O(l), a flammable compound that wasonce used as a surgical anesthetic, has the structure H3C-CH2- O- CH2-0 CH3 The complete combustion of 1 mol of C4H10O1l2 to CO21g2and H2O(l) yields ΔH° = -2723.7 kJ. (a) Write a balancedequation for the combustion of 1 mol of C4H10O(l). (b) Byusing the information in this problem and data in Table 5.3,calculate ΔHf° for diethyl ether.Estimate the enthalpy change for the combustion of one mole of acetylene, C2H2, to form carbon dioxide and water vapor. 2C2H2(g) + 5O2(g) ⟶⟶ 4CO2(g) + 2H2O(g) BE(C–H) = 456 kJ/molBE(C≡C) = 962 kJ/molBE(O=O) = 499 kJ/molBE(C=O) = 802 kJ/molBE(O–H) = 462 kJ/mol Group of answer choices A.) +653 kJ/mol B.) –1010 kJ/mol C.) –1759 kJ/mol D.) –155 kJ/mol E.) +1010 kJ/mol
- When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide, NO. Calculate ΔH∞rxn for the reaction below using the following information; ΔH∞f [NH3(g)] = -45.9 kJ/mol; ΔH∞f [NO(g)] = 90.3 kJ/mol; ΔH∞f [H2O(g)] = -241.8 kJ/mol. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
- Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: 4HCl(g) + O2(g) ---> 2Cl2(g) + 2 H2O(g) Please answer fast i give upvote .Liquid carbon disulfide burns in the presence of oxygen to produce two gaseous combustion products, carbon dioxide and sulfur dioxide. Species DHf° (kJ/mol) DGf° (kJ/mol) CS2 (g) 117.4 65.3 CS2 (l) 89.7 65.3 O2 (g) 0.00 0.00 CO2 (g) - 393.5 - 394.4 SO2 (g) - 296.9 - 300.4 Write a balanced equation for this reaction. 2. Calculate the values of ΔH°rxn and ΔG°rxn for this reaction 3. Is this reaction exothermic or endothermic? Liquid carbon disulfide is vapourised to gaseous carbon disulfide. Calculate the value of ΔS°vap for of liquid carbon disulfide at 25°Some bacteria can obtain energy for growth by oxidizing ethanol, first to acetaldehyde and then acetic acid. Calculate ΔH° for the reaction:(a) C2H5OH(l) + ½O2(g) ---> CH3CHO(l) + H2O(l)Use the following enthalpies of combustion: ΔcH°(C2H5OH, l) = -1362.8 kJ mol-1, ΔcH°(CH3CHO, l) = -886.8 kJ mol-1
