FeS 2 ( s ) + O 2 ( g ) SO 2 ( g ) + Fe 2 O 3 ( s )[unbalanced] Be sure to answe
ID: 979644 • Letter: F
Question
FeS2(s) + O2(g) SO2(g) + Fe2O3(s)[unbalanced]
Be sure to answer all parts.Sulfur dioxide is used to make sulfuric acid. One method of producing it is by roasting mineral sulfides. For example,
FeS2(s) + O2(g) SO2(g) + Fe2O3(s)[unbalanced]
A production error leads to the sulfide being placed in a 950L vessel with insufficient oxygen. The partial pressure of O2 is 0.53 atm, and the total pressure is initially 1.05 atm, with the balance N2. The reaction is run until 85% of the O2 is consumed, and the vessel is then cooled to its initial temperature. What is the total pressure and partial pressure of each gas in the vessel?
? atm N2 ? atm unreacted O2 ? atm SO2 ? atm total
Explanation / Answer
Balanced equation,
4FeS2(s) + 11O2(g) ---> 8SO2(g) + 2Fe2O3(s)
Initial O2 pressure = 0.53 atm
85% of it reacted, that is = 0.85 x 0.53 = 0.45 atm
Remaining O2 = 0.15 x 0.53 = 0.08 atm
N2 initial pressure = 1.05 - 0.53 = 0.52 atm remains unchanged
SO2 pressure = 0.45 x 8/11 = 0.33 atm
Total pressure = 0.08 + 0.52 + 0.33 = 0.93 atm
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