Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe2O3) is:
4 Fe(s) + 3 O2(g) →2 Fe2O3(s) |
ΔHrxn = −1.65 ×103 kJ |
(a) What is the ΔHrxn
when 0.250 kg of iron rusts? (Answer in kJ)
(b) How much rust forms when 7.40 x 103 kJ of
heat is released? (Answer in g of
Fe2O3)
Get Answers For Free
Most questions answered within 1 hours.