Use bond enthalpies in the table below to estimate AH for each of the following reactions. I Review Constants Periodic Table Part A Average bond enthalpy (kJ/mol) C-H: 413 N-H: 391 O-H: 463 F-F: 155 Br Br C-C: 348 N-N: 163 O-0: 146 Br-C-H + Cl-Cl - Br-C-Cl + Cl-H C=C: 614 N-O: 201 0=0: 495 Cl-F: 253 C-N: 293 N-F: 272 0-F: 190 Cl-Cl: 242 Br Br C-0: 358 N-Cl: 200 O-Cl: 203 Br-F: 237 234 Br-Cl: 218 Br-Br: 193 C=0: 799 N-Br: 243 0-I: Express your answer in kilojoules to three significant figures. C-F: 485 H-H: 436 C-Cl: 328 H-F: 567 C-Br: 276 H-Cl: 431 I-Cl: 208 kJ 202.3 240 H-Br: 366 H-I: 299 I-Br: 175 ΔΗ- C-I: I-I: 151 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining Part B H. H-C-H +2 0=0- 0=C=0+ 2 H-O-H

Using bond enthalpies in the table, estimate AH for the following gas-phase reactions. Average Bond Enthalpies (kJ/mol) Single Bonds C-H C-C C-N C-O C-F C-Cl C-Br C-I C-S 413 |N-H 348 |N-N 293 N-O 358 |N-F 485 |N-Cl 328 N-Br 243 276 240 259 CH–C1 242 193 Br-Br Multiple Bonds C=C C=C C=N C=N 614 839 615 391 O-H 0-0 163 201 O-F 272 O-Cl 200 O-I 201 463 146 190 203 234 339 H-H S-H 436 S-F 567 S-Cl 327 253 H-F H-Cl 431 S-Br 218 H-Br 366 S-S 266 H-I 299 |N=N 418 0=0 |N=N 941 |N=O 607 495 Part C Estimate AH for the reaction. Express your answer using one significant figure. AH = Submit —| ΑΣΦ Provide Feedback H H-N-N-H+CI-CI-2 H-N-CI -H+C₁_a_ Previous Answers Request Answer HH X Incorrect; Try Again; 3 attempts remaining ? kJ

Calculate the heat of reaction for

Given the reaction: ½ H2 (g) + ½ Cl2 (g) --> HCl (g)                ΔH = -92 kJ/mol What is the missing bond energy in kJ/mol?                                                 H - H      BE = 435 kJ/mol                                                 H - Cl     BE = 431 kJ/mol                                                 Cl - Cl     BE = ? kJ/mol? A) 96 B) 335 C) 188 D) 88 E) 243

Q/ For each compound below, write the balanced chemical equation that represents its enthalpy of formation (ΔHf ° ). a) Li2CO3(s) b) CH3CH2OH(l)

Given the following thermochemical equation, what is the standard heat of formation for NaOH? 2NaOH(s)-->2Na (s) + O2 (g) + H2 (g) TriangeH= +875.6 kJ a) 875.6 kJ b) -875.6 kJ c) 437.6 kJ d) -437.6 kJ e) 1751.1 kJ f) -1751.1 kJ

Calculating the heat of reaction from bond energies Calculate the heat of reaction AH for the following reaction: 2 H₂(g) + O₂(g) → 2 H₂O(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ mol X 1/5

eats of formation given in the table: ! Formula C₂H2(g) 226.7 NH3(g) -46.19 C6H6(1) 49.0 ate CaCo3(s) -1207.1 -635.5 CaO(s) CO2(g) AH f (kJ/mol) ide CO(g) C(s) -393.5 -110.5 1.88 C₂H6(8) -84.68 C₂H5 OH (1) -277.7 C₂H4(8) 52.30 C6H12O6 -1273 Substance OA Hrxn = 327.6 kJ/mol OA Hrxn = -163.8 kJ/mol OAHrxn = -327.6 kJ/mol OA Hrxn = 56.1 kJ/mol OA Hrxn = 163.8 kJ/mol Hydrogen chloride Hydrogen fluoride Hydrogen iodide Methane Methanol Propane Silver chloride Sodium bicarbonate Sodium carbonate Sodium chloride Sucrose Water (s) nide HBr(g) -36.23 Water vapor :a, determine the enthalpy change for the reaction: 2 CH4(g) + O₂(g) 2 CH3OH(e) Formula AH f (kJ/mol) HCI(g) HF(g) HI(g) 25.9 CH4(g) -74.80 |CH3 ОН -238.6 (1) C3H8(g) -103.85 -127.0 AgCl(s) NaHCO3 (s) C12H22O11130.9 (s) NaCl -92.30 -268.60 -947.7 -410.9 C12H22O11221 (s) H₂O(l) -285.8 H₂O(g) -241.8

The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize.     a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water.      C3​H8​(g)+    O2​(g) ---->CO2​(g)+     H2​O(g)   b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite.  3C(s,graphite)+4H2​(g)--->C3​H8​(g) ΔHo = -103.8 kJ/mol   C(s,graphite)+O2​(g)--->CO2​(g) ΔHo= -393.5 kJ/mol   H2​(g)+1/2​ O2​(g)--->H2​O(g) ΔHo= -285.8 kJ/mol      kJ/mol…

Determine the enthalpy change for  combustion of using bond energies for             2C2H6(g)  + 7O2(g)  ➜ 4CO2(g)  + 6H2O(l) see image