Calculate the mass of H2O produced by metabolism of 1.2 kg of fat, assuming the fat consists entirely of tristearin (C57H110O6), a typical animal fat, and assuming that during metabolism, tristearin reacts with O2 to form only CO2 and H2O.

1,7Kg of is produced

Explanation:

Balanced chemical reaction

To find the mass of produced in a reaction, we need to start by identifying that chemical reaction and balancing it.

The question give us the reactants and the products, do we know:

+ ⇒ +

Counting C, H and O in reactants and products; and balancing them with stoichiometric coefficients, we have that the balanced chemical equation is:

2 + 160 ⇒ 114 + 110

Stoichiometry

The question says us that 1.2 Kg of fat () react.

To find the amount of we need to find the moles of . The way to do it, is using the molar mass:

Taking the molar mass of each element in the periodic table, multiplying by the subscript and adding all the partial values:

The moles of that react are:

The balanced chemical reaction tell us that each 2 moles of that react, produce 110 moles of . It means that:

1.6826 mol mol

Finally, using the molar mass of , we can find its mass:

92.543 mol =1665.7 g  

With two sig figs, the mass:

1665.7g ≅ 1.7 Kg

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