Question
Asked Oct 18, 2019

Iron can be converted to Fe2O3 according to the reaction below. How much heat (in kJ) is required to convert 10.5 g of iron to Fe2O3?

2Fe(s) + 3CO(g) → Fe2O3(s) + 3CO2(g)  ΔH = 26.8 kJ/mol

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Expert Answer

Step 1

Iron can be converted to Fe2O3 according to the given reaction. Amount of heat (in kJ) required to convert 10.5 g of iron into Fe2O3 is to be calculated.

2Fe(s)3CO (g) -»
ДН. — 26.8 kJmol
Fe,O, (s) + 3со, (в)
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2Fe(s)3CO (g) -» ДН. — 26.8 kJmol Fe,O, (s) + 3со, (в)

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Step 2

Calculate the moles of Fe in 10.5 g of iron-

As per the balanced equation, 2 moles of Fe needs 26.8 KJ of heat to convert to Fe2O3.

Thus, first convert 10.5 g of Fe into moles of Fe.

Given Mass of Fe
10.5 g
Moles of Fe
55.845 g/mol
Molar mass of Fe
. Moles of Fe = 0.188 moles
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Given Mass of Fe 10.5 g Moles of Fe 55.845 g/mol Molar mass of Fe . Moles of Fe = 0.188 moles

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Step 3

Calculate the amount of heat (in kJ) required to convert 0....

Heat required by 2 moles of Fe to convert to Fe, O, = 26.8 KJ
Thus, heat required by 0.188 moles of Fe to convert to Fe,0
0.188 moles
26.8KJX
= 2.52 KJ
2 moles
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Heat required by 2 moles of Fe to convert to Fe, O, = 26.8 KJ Thus, heat required by 0.188 moles of Fe to convert to Fe,0 0.188 moles 26.8KJX = 2.52 KJ 2 moles

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