Using the values of bond energy from the table below, estimate the enthalpy change for the following reaction: C₂H4 (9) + H₂O2(g) → CH₂OHCH₂OH(g) Bond Bond Energy (kJ/mol) C=C 602 0-0 146 C-C 346 C-O 358 AHrxn = kJ

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.

Use the average bond enthalpies from Table 8.3 in your textbook to estimate ΔHΔH for the formation of CO2(g) by the following reaction:                                 CH4(g) + 2O2(g) --> CO2(g) +2H2O(g)

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

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The enthalpy change for the following reaction is 66.4 kJ. Using bond energies, estimate the N=O bond energy in NO2(g).N2(g) + 2O2(g)2NO2(g) ____kJ/mol

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

The heat of reaction for a chemical reaction can be calculated by finding the sum of the bond energies of the products and subtracting that from the sum of the bond energies of the reactants: Heat of reaction==Sum of the energy for the bonds broken − Sum of the energy for the bonds formedSum of reactant bond energies − Sum of product bond energiesHeat of reaction=Sum of the energy for the bonds broken − Sum of the energy for the bonds formed=Sum of reactant bond energies − Sum of product bond energies When calculating the sum of the bond energies, each bond in the reaction must be accounted for. For example, CH4CH4 is a reagent with a coefficient of 1 in the reaction. There are four C−HC−H bonds in methane and one methane molecule per reaction, for a total of four C−HC−H bonds on the reactant side. All four bonds must be accounted for when finding the sum of the bond energies for the reactants. Calculate the heat of reaction using the average bond dissociation energies given in the…

CH, Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. AH (kJ/mol) Bond H-O C-C H-C 010 C- 010 + H₂O(g) → CH₂CH(OH)CH₂(g) Enthalpy change 44 Submit Substance 463 610 413 346 358 bCalculate the enthalpy change for this reaction from enthalpies of formation. AƒH (kJ/mol) la 272.8

Using the bond energies as shown, determine the approximate enthalpy change for each of the following reactions:(a) Cl2(g) + 3F2(g) ⟶ 2ClF3(g)(b) H2 C = CH2(g) + H2(g) ⟶ H3 CCH3(g)(c) 2C2 H6(g) + 7O2(g) ⟶ 4CO2(g) + 6H2 O(g)