Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g)

Question

Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction

2 SO2 (g) + O2 (g) ---> 2 SO3 (g)

The standard enthalpies of formation of SO2 (g) and SO3 (g) are:

* for S02 = - 296.8 kJ/mol

*for SO3 = - 395.7 kJ/mol

Calculate the amount of energy in the form of heat that is produced when a volume of 4.70 L of SO2 (g) is converted to 4.70 L of SO3 (g) according to this process at a constant pressure and a temperature of 1.00 bar and 25 degree celsius. Assume ideal gas behavior.

Show work please

Explanation / Answer

dHo for the reaction,

dHo = dHo(products) - dHo(reactants)

       = (2 x -395.7) - (2 x -296.8)

       = -197.8 kJ/mol

moles SO2 reacted = PV/RT

P = 1 bar = 1 atm

V = 4.70 L

R = gas constant

T = 25 + 273 = 298 K

So,

moles SO2 = 1 x 4.70/0.08206 x 298 = 0.192 moles

amount of energy produced = 0.192 moles x -197.8 kJ/mol = -38.0 kJ/mol

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