3. Pyrite (FeS2), aka Fool's Gold, can break down in the presence of oxygen gas to form various iron oxides, iron sulfates, and sulfur dioxide gas. The reaction below is just one possibility. Given the following information: 2FES2(s) + 502(g)→ 2FE0(s) + 4S02(g) AH", = -1370 kJ/mol,pxn rxn AHƒ for SO2(g) = AH; for Fe0(s) = -297 kJ/mol -268 kJ/mol (a) Calculate the standard heat of formation, AH,E, for FeS,(s). (b) Is the formation of FeS2(s) from elements in their pure form endothermic or exothermic. How do you know? (c) If 137 g of FeS, are attacked by 02 molecules in the atmosphere, calculate the amount of heat absorbed or released. (d) Interestingly, iron is NOT oxidized or reduced by this reaction. Which atom is? Determine the oxidation numbers of that element on both sides of the equation

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3. Pyrite (FeS,), aka Fool's Gold, can break down in the presence of oxygen gas to form various iron
oxides, iron sulfates, and sulfur dioxide gas. The reaction below is just one possibility. Given the
following information:
2FES2(s) + 502(g) → 2Fe0(s) + 4S02(g)
ΔΗ .
= -1370 kJ/molpxn
rxn
AH; for SO2(g) =
AH; for FeO(s) =
-297 kJ/mol
-268 kJ/mol
(a) Calculate the standard heat of formation, AHfº, for FeS2(s).
(b) Is the formation of FeS2(s) from elements in their pure form endothermic or exothermic.
How do you know?
(c) If 137 g of FeS, are attacked by 0, molecules in the atmosphere, calculate the amount of
heat absorbed or released.
(d) Interestingly, iron is NOT oxidized or reduced by this reaction. Which atom is? Determine
the oxidation numbers of that element on both sides of the equation
Transcribed Image Text:3. Pyrite (FeS,), aka Fool's Gold, can break down in the presence of oxygen gas to form various iron oxides, iron sulfates, and sulfur dioxide gas. The reaction below is just one possibility. Given the following information: 2FES2(s) + 502(g) → 2Fe0(s) + 4S02(g) ΔΗ . = -1370 kJ/molpxn rxn AH; for SO2(g) = AH; for FeO(s) = -297 kJ/mol -268 kJ/mol (a) Calculate the standard heat of formation, AHfº, for FeS2(s). (b) Is the formation of FeS2(s) from elements in their pure form endothermic or exothermic. How do you know? (c) If 137 g of FeS, are attacked by 0, molecules in the atmosphere, calculate the amount of heat absorbed or released. (d) Interestingly, iron is NOT oxidized or reduced by this reaction. Which atom is? Determine the oxidation numbers of that element on both sides of the equation
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