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?

Question

Chemistry

Scott Ferguson

27 May, 08:28

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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Answers (1)

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Reece Shepard · Answer 1

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