Sulfur dioxide, SO_2(g), can react with oxygen to produce sulfur trioxide, SO_3(

Question

Sulfur dioxide, SO_2(g), can react with oxygen to produce sulfur trioxide, SO_3(g), by the following reaction 2SO_2(g) + O_2(g) rightarrow 2SO_3(g) The standard enthalpies of formation for SO_2(g) and SO_3 (g) are Delta H degree _f [SO_2 (g)] = -296.8 kJ/mol Delta H degree _f [SO_3 (g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.59 L of SO_2(g) is converted to 4.59 L of SO_3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 degree C. Assume ideal gas behavior.

Explanation / Answer

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

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

DeltaH {SO2(g)}=-296.8 kJ/mol
DeltaH {SO3(g)}=-395.7 kJ/mol
Using equation PV = nRT
Number of moles of 4.59 L of SO2 = PV/RT = 1.00 x 4.59/0.0821 x 298 = 0.1876
And No. of moles of 4.59 L of SO3 are also 0.1876
Now the enthalpies of formation for 0.1876 moles of SO2(g) and SO3(g) are:
0.1876 x (-296.8) and 0.1876 x (-395.7) respectively.
Hence the amount the amount of energy in the form of heat that is produced when a volume of 4.59 L of SO2(g) is converted to 4.59L of SO3(g) = 0.1876 x {-395.7 - (-296.8)} = 0.1876 x (-98.9) = -18.55364 kJ

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.