We are asked to calculate the volume of O2(g) needed to completely convert 5.00 g sulfur to sulfur trioxide. We can calculate the volume of the gas using the ideal gas equation:
P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K
In the ideal gas equation, the amount of O2 in moles is needed but the moles of sulfur is given instead. We will have to calculate the moles of O2 from S first using a balanced overall reaction equation and mole to mole comparison.
Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid.
S(s) + O2(g) → SO2(g)
2SO2(g) + O2(g) → 2SO3(g)
What volume of O2(g) at 350.°C and a pressure of 5.25 atm is needed to completely convert 5.00 g sulfur to sulfur trioxide?
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.