∆ H o

a)   The following reaction occurs in an open beaker: C2H5OH (g) --->  C2H4(g) +  H2O (g)         {Bond Energy  (kJ/mol): C-H = 415 ;   C-C = 345 ;   C-O = 350 ;   O-H = 464 ;   C=C = 611}i)    Calculate the ΔH0rxn for this reaction from the given bond energies.  kJ ii)   Is this reaction an open, closed or isolated system? iii)  Would you feel hot or cold if you were near this reaction when it occurred?        This is because (choose from I - V)  I.     the reaction is exothermic and absorbs energy from the surroundings. II.   the reaction is exothemic and releases energy to the surroundings. III.  the reaction is endothermic and absorbs thermal energy from the surroundings. IV.   the reaction is endothermic and loses heat to the surroundings. V.    the reaction produces steam which contains a lot of heat.

Calculate the enthalpy of combustion of ethene, C2H4, given the bond energies in Table 1 below. C2H4 (g) + O2 (g) CO2 (g) + H2O () Table 1. Bond Energies of Selected Bonds. Bond Bond Energy (KJ/mol.) C-H 413 C=C 614 O=O in O2 498 C=O in CO2 799 O-H 467 O 947 KJ O -1494 KJ O 3196 KJ O -2266 KJ

The enthalpy change for the following reaction is -92.2 kJ. Using bond energies, estimate the H-H bond energy in H₂(g). N₂(g) + 3H₂(g) → 2NH3 (9) Bond Bond Energy (kJ/mol) N=N N-H Bond energy = 945 391 kJ/mol

Determine the enthalpy of reaction for the following: CH₂=CH2(g) + H2(g) → CH3CH3(g)

The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF₂(g) + H₂O(g) → O₂(g) + 2HF(g) ΔΕ. = = -318 kJ rxn Using bond energies, calculate the bond dissociation energy of the O-F bond in OF2. Average Bond Energies (kJ/mol) Single Bonds H-H H-F H-CI H-Br H-1 C-H C-C C-N -0 -F C-Cl C-Br C-1 C-S 432 565 427 363 295 413 347 305 358 485 339 276 240 259 *C = O(in CO₂) = 799 N-H N-N N-F N-CI N-Br N-O O-H 0-0 O-F O-CI 0-1 F-F F-CI F-Br CI-CI Cl-Br Br-Br O-F bond dissociation energy = 391 160 272 200 243 201 467 146 190 203 234 154 253 237 239 218 193 kJ/mol H I-CI 1-Br S-H S-F S-CI S-Br S-S Si-Si Si-H Si-C Si-O 149 208 175 347 327 253 218 266 340 393 360 452 Multiple Bonds C=C C=C 0=0 =0* C=O N=O N=N N=N C=N CIN 614 839 495 745 1072 607 418 941 891 615

Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation   NH3 (g) + 2 O2 (g) --> HNO3 (g) + H20 (g)  Average molar bond enthalpies. (?bond) Bond ??⋅???−1 Bond ??⋅???−1 O−H 464 C≡N 890 O−O 142 N−H 390 C−O 351 N−O 201 O=O 502 N=N 418 C=O 730 N=O 607 C−C 347 F−F 155 C=C 615 Cl−Cl 243 C≡C 811 Br−Br 192 C−H 414 H−H 435 C−F 439 H−F 565 C−Cl 331 H−Cl 431 C−Br 276 H−Br 368 C−N 293 H−S 364 C=N 615 S−S 225

For the reaction: 2C4H10(g)  13O2(g) + 8CO2(g )+ 10H2O(g) Part 1) Predict the enthalpy of reaction from the average bond enthalpies. Be sure your answer has the correct number of significant digits. Note: Reference the Bond energies table for additional information. =ΔHorxn kJmol Part 2)  Calculate the enthalpy of reaction from the standard enthalpies of formation of the reactant and product molecules. Be sure your answer has the correct number of significant digits. Note: Reference the Thermodynamic properties of pure substances table for additional information. =ΔHorxn kJmol     Pls help me with this question asap!!!

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Calculate the ΔHrxn using bond enthalpies for the balanced equation below (Lewis structures also provided).   Bond Enthalpy Values: Bond ΔH (kJ/mol) C=C 611 C–H 414 H–H 436 C–C 347 Group of answer choices -219 kJ -128 kJ 286 kJ -564 kJ