• Use the table of Bond Energies (BE) in the table below to calculate the Heat of Reaction, AHxn for the complete combustion of two moles of liquid ethanal (CH3CHO (1): 2 CH3CHO () + 5 02(9) → 4 CO2 (g) + 4 H20(9) AHrxn kJ H 0 =0 0=C=0 H-C-C H. H-O-H TABLE 9.5 Bond Energies (in kJ/mol)* Single Bonds H N F CI Br H 432 C 411 346 386 305 167 459 358 201 142 S 363 272 226 F 565 485 283 190 284 155 CI 428 327 313 218 255 249 240 Br 362 285 201 217 249 216 190 I 295 213 201 278 208 175 149 Multiple Bonds C=C 602 C=N 615 c=0 745 (799 in CO,) C=C 835 C=N 887 C=0 1072 N=N 418 N=O 607 S=0 (in SO,) 532 N=N 942 0=0 494 S=0 (in SO,) 469 *Data are taken from J. E. Huheey, Keiter, and Keiter, Inorganic Chemistry, 4th ed. (New York: HarperCollins, 1993), pp. A21-A34. AHxa = ( Select ) v kJ / (2 mol CH3CHO (1) ) Use the: • Heat of Reaction AHrxn values for the combustion of two moles of liquid ethanal (CH3CHO () • the Enthalpies of Formation (AH;º) for carbon dioxide (CO2(9)) and water (H20(9) to calculate the: • Enthalpy of Formation (AHF° ) of 1 mole of liquid ethanal (CH3CHO (1) ): AH;° = ISelect] v kJ/mol CH3CHO (1) Enthalpies of Formation: CO2(g) AHf° = - 393.5 kJ/mole H20(g) AH:° = - 241.8 kJ/mole

3. Draw and label a PE diagram for the reaction 2 NOBr (g->2 NO(g) + Br2(g) + 50 kJ, in which Ea(f) = 30 kJ

According to the reaction below what is the value of KKJ for the complete combustion of 1.00 g of CH4g?

Pls help ASAP

Use your table of Heats of Formation to calculate the heat of reaction for the following reaction: C2H4(g)  +  3O2(g)  ⟶   2CO2(g)  + 2H2O(g)

cellus_engine.html?ClassID=527350766# 1.00 g of sucrose, C12H22O11, reacts with excess oxygen in a bomb calorimeter with a heat capacity of 12.5 kJ/°C. The initial temperature is 22.0 °C and the final temperature is 23.3 °C. What is the enthalpy of the reaction? AH: [?] kJ/mol Enter either a + or - sign AND the magnitude. Do not round until the end. Use significant figures. AH, rxn (kJ/mol) Enter

When a 7.41-g sample of solid potassium chlorate dissolves in 59.3 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 22.00 oC to 12.96 oC. Calculate H in kJ/mol KClO3 for the solution process. KClO3(s)  K+(aq) + ClO3-(aq)   The specific heat of water is 4.18 J/g-K.Hsolution = _________ kJ/mol KClO3.