Question

In: Chemistry

Given the following bond-dissociation energies, calculate the average bond enthalpy for the Ti-Cl bond.

Given the following bond-dissociation energies, calculate the average bond enthalpy for the Ti-Cl bond.

AH(kJ/mol) TiCl4(g) TiCl;(g) TİC,(g) TICI(g) TiCl3(g) + Cl(g) TİCI,(g) + CI(g) TiCI(g) + CI(g) Ti(g) + CI(g) 335 423 444 519

 

 

Solutions

Expert Solution

Average bond energy of Ti-C1 bond:

 

TiC14(g) → TiC13(g) + C1(g) ΔH = 335kJ

TiCl3(g) → TiCl2(g) + Cl(g) ΔH = 423 kJ

TiCl2(g) → TiCl(g) + Cl(g) ΔH = 444 kJ

TiCl(g) → Ti(g) + Cl(g) ΔH = 519 kJ

 ΔH = 1721 kJ

 

Average Ti-Cl bond = 1721 kJ/4

                                   = 430.25 kJ

 

Average bond enthalpy of Ti-Cl = 430 kJ.

Average bond energy of Ti-C1 bond:

 

TiC14(g) → TiC13(g) + C1(g) ΔH = 335kJ

TiCl3(g) → TiCl2(g) + Cl(g) ΔH = 423 kJ

 

Junaid answered 2 years ago
Next > < Previous

Related Solutions

Use average bond energies to estimate the enthalpy changes of the following reactions: a. N2(g) +...
Use average bond energies to estimate the enthalpy changes of the following reactions: a. N2(g) + 3 H2(g) -> 2 NH3(g) b. N2(g) + 2 H2(g) -> H2NNH2(g) c. 2 N2(g) + O2(g) -> 2 N2O(g)
Calculate ΔH0 rxn for the following reaction using given bond energies: C3H8 + 5 O2 →...
Calculate ΔH0 rxn for the following reaction using given bond energies: C3H8 + 5 O2 → 3 CO2 + 4 H2O C-H: 413 kJ/mol, C-C : 347 kJ/mol, O=O : 498 kJ/mol , C=O : 799 kJ/mol, O-H: 467 kJ/mol
The enthalpy change for the following reaction is -136 kJ. Using bond energies, estimate the H-O...
The enthalpy change for the following reaction is -136 kJ. Using bond energies, estimate the H-O bond energy in H2O2(g). H2(g) + O2(g) --> H2O2(g)
The bond dissociation energy of a typical C-Cl bond in a chlorofluorocarbon is approximately 330 kJ/mol....
The bond dissociation energy of a typical C-Cl bond in a chlorofluorocarbon is approximately 330 kJ/mol. (a)    Write the equation for the photodissociation of the chlorine atom from chlorotrifluoromethane. (2 pts) (b)    What range of wavelengths of photons is able to cause the reaction you have written in part (a)? (4 pts) (c)    Describe how the product of the reaction in part (a) leads to an increase in the decomposition of stratospheric ozone. Provide a reaction mechanism to support your answer. (4 pts)
#1. Estimate ΔH for the reaction using bond dissociation energies. Give your answer in kcal. C6H12O6...
#1. Estimate ΔH for the reaction using bond dissociation energies. Give your answer in kcal. C6H12O6 has five C−C bonds, seven C−H bonds, seven C−O bonds, and five O−H bonds. #2. Is the reaction exothermic or endothermic? #3. The following equation shows the conversion of aluminum oxide (from the ore bauxite) to aluminum: 2Al2O3(s)→4Al(s)+3O2(g),   ΔH = +801.0 kcal ----> a. Is the reaction exothermic or endothermic?
Use bond-energy data to calculate the enthalpy of formation for eah of the following compounds at...
Use bond-energy data to calculate the enthalpy of formation for eah of the following compounds at 25 C a) n-Octane, C8H18(g) b) Napthalene, C10H8(g) c) Formaldehyde, H2CO(g) d) Formic acid, HCOOH(g) Give the most likely reason for the largest discrepancies between your calculated values and the ones in the tables.
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following...
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s) H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall reaction : CH4(g) + 2 O2 (g) ------> CO2(g) + 2H2O(l) 2H2O(l) ------> 2H2O(g) ∆H = 88 kJ CH4(g) + 2 O2 (g) ------> CO2(g) + 2H2O(g) ------> 2O(g) ∆H = -802 kJ
Calculate the enthalpy change for: C2H4 (g) + H2 (g) ---> C6H6 (l) given the following:...
Calculate the enthalpy change for: C2H4 (g) + H2 (g) ---> C6H6 (l) given the following: C2H4 (g) + 3O2 (g) ---> 2CO2 (g) + 2H2O(l) deltaH= -845.2kJ 2H2(g) + O2 (g) ---> 2H2O(l) deltaH= -573.2kJ 2C2H6(l) + 7O2(g) ---> 2CO2 (g) + 6H2O(l) deltaH= 1.1987.4kJ
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall reaction : NO(g) + O (g) ------? NO2(g) 2O3(g) ------? 3O2(g) ?H = - 427 kJ O2(g) ------? 2O(g) ?H = 495 kJ NO(g) + O3 (g) ------? NO2 (g) + O2 (g) ?H = - 199 kJ
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT