Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO2(g), by the reaction 2SO2(g) + O2(g)2 → SO3(g)

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

ΔHf= [SO2(g)] = -296.8 kJ/mol
ΔHf= [SO2(g)] = -395.7 kJ/mol

Calculate the amount of energy in the form of heat that is produced when a volume of 1.64 L of SO2(g) is converted to 1.64 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C . Assume ideal gas behavior.

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

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