waLLESS Important values if needed for this question. Using the values of bond energy from the table below, estimate the enthalpy change for the following H₂(g) + O₂(g) → H₂O₂(g) AH = Bond Bond Energy (kJ/mol) H-H 0=0 0-0 H-O kJ AHxn vai needed for this que Using average bond enthalpies, estimate the enthalpy change for the following reaction: Cl₂(g) + F2 (g) → 2C1F (g) 436 498 146 463 Bond Bond Energy (kJ/mol) CI-CI F-F CI-F kJ 242 155 253

Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)X2O4 has a structure ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 470.5 kJ/molΔHof of X2O4(g) is 11 kJ/molThe X-X single bond energy is 148 kJ/molUse the above data to estimate the average  bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.

Calculate the standard enthalpy change for the following reaction: CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) O-243 kJ/mol O 188 kJ/mol O 166 kJ/mol O-802 kJ/mol O-166 kJ/mol

Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO

: : Use the bond energies in the table to estimate the enthalpy of reaction for the formation of sulfur tetrafluoride monoxide. Bond Energy (kJ/mol) S-F 310 S-O 265 S=0 523 0-0 142 O=0 498 O-F 180 AHTXN = kJ/mol

c) TABLE 2 shows several selected thermochemical data. TABLE 2 AH (kJ mol-') Entahlpy Lattice energy of sodium oxide Enthalpy of formation of sodium oxide First ionisation energy of sodium First electron affinity of oxygen Second electron affinity of oxygen Enthalpy of atomization of oxygen -2570.0 -415.9 +495.9 -141.0 +791.0 +247.0 Based on the data in TABLE 2, i. construct the Born-Haber cycle. ii. calculate the enthalpy of atomisation of sodium

Use the table provided to estimate AH for the reaction O3 (g) + O (g) →2 O2 (g). Does this reaction consume or produce heat? Single Bond Energies (kJ/mol of bonds) N OS H. F Cl Br I Н 436 C 413 346 N 391 305 163 O 463 358 201 146 S 347 272 226 F 565 485 283 190 284 155 Cl 432 339 192 218 255 253 242 Br 366 285 201 217 249 216 193 I 299 213 201 278 208 175 151 Multiple Bond Energies (kJ/mol of bonds)_ C=C 602 C=N 615 C=O 799 C=C 835 CEN 887 C=O 1072 N=N 418 N=O 607 NEN 945 O=0 498

In each row, pick the compound with the bigger lattice energy. Note: lattice energy is always greater than zero. Which compound has the bigger lattice energy? Be O Li₂O O Cas O NaCt O X O CaCl₂ NaF O

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

Predict the enthalpy of reaction from the average bond enthalpies for the following reaction: 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)  Bond Enthalpy (kJ/mol) H―H 436.4 H―O 460 C―H 414 C―C 347 C═C 620 C―O 351 O―O 142 O═O 498.7 C═O 745 C═O(in carbondioxide) 799 ______ kJ