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) ∆H = -1.65x103 kJ (a) How much heat is released when 0.250 kg of iron rusts? (b) How much rust forms when 4.85x103 kJ of heat is released?
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) ∆H = -1.65x103 kJ (a) How much heat is released when 0.250 kg of iron rusts? (b) How much rust forms when 4.85x103 kJ of heat is released?
General Chemistry - Standalone book (MindTap Course List)
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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) ∆H = -1.65x103 kJ
(a) How much heat is released when 0.250 kg of iron rusts?
(b) How much rust forms when 4.85x103 kJ of heat is released?
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