Answered

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) ΔH = -1.65×10³kJ
(a) How much heat is released when 0.250 kg of iron rusts?

Answer :

tanisharawat014

When 0.250kg 0f iron rusts , 1871kj of heat is released .

Given that ,

Deterioration of buildings ,bridges and other structures through the rusting of iron costs millions of dollars a day .

[tex]4Fe (s) + 3O_{2} (g) -- > 2Fe_{2} O_{3} (s)[/tex]

Enthalpy change of the heat of formation of the reaction is given by ,

delHrxn =-1650kj

Now , molar mass of the iron  =55.845g

molar mass of 4moles of iron = 55.845(4) =223.38g

for 223.38g of iron rusts heat released = 1650kj

thus 250 g of iron rusts heat released = 1650kj ( 250g) /223.38g=1871kj

Hence , 1871kj heat is released when 0.250 kg of iron rusts.

Learn more about heat release here :

brainly.com/question/16412313

#SPJ4

Other Questions