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11 Dec 2019

A high temperature reaction vessel is charged with 0.5860 mol of iron powder and 35.1 L of oxygen gas at STP.

4Fe(s) + 3O2(g) yields 2Fe2O3(s)

After the reaction vessel is cooled, and assuming reaction goes to completion, what volume of oxygen remains?

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13 Dec 2019
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Related questions

The chemical reaction that causes iron to rust in air is given by

4Fe+3O2?2Fe2O3

in which

?Hrxn? =?1648.4 kJ
?Srxn?

=?543.7 J/K

1. What is the Gibbs free energy for this reaction at 3200 K? Assume that ?H and ?S do not change with temperature.

2. At what temperature Teq do the forward and reverse rusting reactions occur in equilibrium?

Iron ore is converted to iron metal in a reaction with carbon. 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g) If 5.13 moles of Fe2O3 are used, what amount of C is needed and what amounts of Fe and CO2, in moles, are produced?

mol C

mol Fe

mol CO2

In the presence of oxygen gas, H2O (?Hf = -285.8 kJ·mol-1) reactsexothermically with elemental sulfur (in its standard state) toform sulfuric acid according to:
S8(s) + 12 O2(g) + 8 H2O(l) ? 8 H2SO4(l) ?Hrxn = -4225.6 kJ.
(a) What is the enthalpy of formation of sulfuric acid?






(b) Assume that the reaction above is conducted in a 53.2 g pyrexglass vessel to form 1.00 mol of H2SO4. What is the temperature ofthe vessel after the reaction if it was at room temperature (21.0°C) before the reaction and all reaction heat was transferred tothe vessel? (Cs, pyrex = 0.753 J·g-1·K-1)


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