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Calculate the standard enthalpy change (ΔH⁰rxn ) for the reaction of TiCl4(g) and H2O(g) to form...

Calculate the standard enthalpy change (ΔH⁰rxn ) for the reaction of TiCl4(g) and H2O(g) to form TiO2(s) and HCl(g) given the standard enthalpies of formation (ΔH⁰f ) shown in the table below. (Include the sign of the value in your answer.)

  kJ

Compound

ΔH⁰f 

(kJ/mol)
TiCl4(g)

−763.2
H2O(g)

−241.8
TiO2(s)

−944.0
HCl(g)

−92.3
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Answer #1

we have:

Hof(TiCl4(g)) = -763.2 KJ/mol

Hof(H2O(g)) = -241.8 KJ/mol

Hof(TiO2(s)) = -944.0 KJ/mol

Hof(HCl(g)) = -92.3 KJ/mol

we have the Balanced chemical equation as:

TiCl4(g) + 2 H2O(g) ---> TiO2(s) + 4 HCl(g)

deltaHo rxn = 1*Hof(TiO2(s)) + 4*Hof(HCl(g)) - 1*Hof( TiCl4(g)) - 2*Hof(H2O(g))

deltaHo rxn = 1*(-944.0) + 4*(-92.3) - 1*(-763.2) - 2*(-241.8)

deltaHo rxn = -66.4 KJ/mol

Answer: -66.4 KJ/mol

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