Sulfuric acid is produced commercially by the reactions indicated below at the appropriate percent yields for each step. The second step utilizes air as a source of oxygen and heats it to 4000C in the presence of vanadium (V) oxide, a catalyst. Assuming air is 21% oxygen by volume, what volume of air at 190C and 754 torr is required to produce enough SO3 to eventually yield 1.00 metric ton (1000kg=1metric ton) of sulfuric acid?
S(s) + O2(g)--->SO2(g) 98.3%
2SO2(g) + O2(g)--->2SO3(g) 94.5%
H2SO4(l) + SO3(g) --->H2S2O7(s) 89.7%
H2S2O7(s) + H2O(l)--->2H2SO4(l) 91.2%
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