Problem: Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction 2SO2(g) + O2(g) → 2SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are ΔH°f [SO2(g)] = -296.8 kJ/mol ΔH°f [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat (kJ) that is produced when a volume of 3.24 L of SO2(g) is converted to 3.24 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0°C. Assume ideal gas behavior.

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

2SO2(g) + O2(g) → 2SO3(g) 

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

ΔH°[SO2(g)] = -296.8 kJ/mol 

ΔH°[SO3(g)] = -395.7 kJ/mol 

Calculate the amount of energy in the form of heat (kJ) that is produced when a volume of 3.24 L of SO2(g) is converted to 3.24 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0°C. Assume ideal gas behavior.