According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4...

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According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4...

According to the following reaction, how much energy is required to decompose 55.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol.

Fe3O4(s) ? 3 Fe(s) + 2 O2(g) ?H°rxn = +1118 kJ

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Answer 1

Answer #1

Hi!

The first step for this problem is to convert our 55.0 kg of Fe3O4 to moles using the molar mass (231.55 grams per mole). Note: we need to convert 55.0 kg to grams first!

Next, we look at the balanced reaction equation given in the problem and see that for every 1 mole of Fe3O4 that is decomposed, +1118 kJ of energy is required. We use this to determine how much energy is required to decompose 237.53 moles:

So, we need 265,558.0 kJ of energy to decompose 55 kg of Fe3O4. That's a lot of energy!

I hope this helps! Please rate if it does : )

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Answer 2

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