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How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s)...

How much energy is evolved during the formation of 197 g of Fe, according to the reaction below?


Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ

A. 964 kJ
B. 1.52 x 103 kJ
C. 3.02 x 103 kJ
D. 482 kJ
E. 8.40 x 103 kJ
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Answer #1

Fe2O3(s) + 2 Al(s) -----> Al2O3(s) + 2 Fe(s) Hrxn = -852KJ

? energy = 197g Fe @ 852kJ / 111.68 (g's of two moles of Fe)

= -1502.95 kJ (exothermic)

1502.95 kJ is released

ans- B 1.52*103 kJ

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