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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?

Melissa Norris

in Chemistry

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Samantha Barber on March 1, 2019

The balanced chemical reaction, we can see that for every 4 moles of Fe (iron), formed, the heat released or heat of reaction is 1.65 x 10^3 kJ. To calculate the moles of iron first:moles of iron = 250 g / (55.85 g/mole) = 4.48 mol So that the heat of reaction is:δhrxn = (-1.65 x 10^3 kJ / 4 mol) * (4.48 mol) = -1.85 kJ


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