(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

What is the heat released by the complete combustion of 22.4x10^3 litres of FeTiH2 - a fuel used in hydrogen cars -, producing liquid water?

2. Relevant equations

ΔH°(reaction) = ΔH°f(products) - ΔH°f(reactants)

3. The attempt at a solution

1 mol FeTiH2 - 22,4 L (STP)

x - 22.4x10^3 litres

x = 1000 moles of FeTiH2

I guess the equation for the combustion is:

1000 FeTiH2(g) + 2250 O2(g) = 1000 H2O(l) + 500 Fe2O3(s) + 1000 TiO2(s)

Using the Hess's Law:

ΔH°(reaction) = 1000ΔH°f(H2O,l) + 500ΔH°f(Fe2O3,s) + 1000ΔH°f(TiO2,s)

- 1000ΔH°f(FeTiH2,g) - 2250ΔH°f(O2,g)

ΔH°(reaction) = - 285800 - 824200 - 945000 - 1000ΔH°f(FeTiH2,g) - 0

I'm having trouble finding the heat of formation of FeTiH2. There're some heat of formation around Google, but I haven't found one at 1 atm pressure. So I guess there must be another way to resolve this problem :tongue:

The answer is - 2.86x10^5 kJ/mol

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# Homework Help: Thermochemical question about the heat of combustion of a hydride

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