Problem: Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars a day. Theactual process requires water, but a simplified equation is4Fe (s) + 3O2 (g) ⟶ 2Fe2O3 (s)             Δ H = −1.65 x 10 3 kJHow much heat is released when 0.250 kg of iron rusts?

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Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars a day. The
actual process requires water, but a simplified equation is

4Fe (s) + 3O2 (g) ⟶ 2Fe2O3 (s)             Δ H = −1.65 x 10 3 kJ

How much heat is released when 0.250 kg of iron rusts?

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Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equations concept. You can view video lessons to learn Thermochemical Equations. Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.