# Problem: 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?

###### FREE Expert Solution

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:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

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.

98% (294 ratings) ###### Problem Details

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 tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. You can view video lessons to learn Gas Stoichiometry. Or if you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

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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.