How much energy is evolved during the formation of 98.7 g of fe, according to the reaction below? fe2o3(s) + 2 al(s) → al2o3(s) + 2 fe(s) δh°rxn = -852 kj?

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20-06-2018
Chemistry

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How much energy is evolved during the formation of 98.7 g of fe, according to the reaction below? fe2o3(s) + 2 al(s) → al2o3(s) + 2 fe(s) δh°rxn = -852 kj?

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kenmyna kenmyna · Answer 1 · 2018-07-04T04:30:07+02:00

kenmyna kenmyna

04-07-2018

The energy that evolved during the formation of 98.7g of Fe is 1505.5 Kj

calculation

find the number of moles of iron = mass/molar mass
molar mass of iron= 55.85 g/mol

moles = 98.7 g /55.85 g/mol = 1.767 moles

energy evolved is therefore = 852 x 1.767 = 1505.5 Kj

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