Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars a day. The actual process also requires water, but a simplified equation is:
$4Fe(s) + 3O_2(g) \rightarrow 2Fe_2O_3(s)$
$\Delta H_{rxn} = -1.65 \times 10^3 kJ$
Be sure each of your answer entries has the correct number of significant figures.
Part 1 of 2
How much heat is released when 0.250 kg of iron rusts?
Part 2 of 2
How much rust forms when $4.10 \times 10^3$ kJ of heat is released?