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 2SO2(g) + O2(g) --> 2SO3(g). The standard enthalpies of formation for SO2(g) and SO3(g) are -296.8 kJ/mol and -395.7 kJ/mol respectively.

Calculate the amount of energy in the form of heat that is produced when a volume 1.12 L of SO2(g) is converted to 1.12 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0C. Assume ideal gas behaviour.

Answer in kJ.

Explanation / Answer

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

deltaH0r = 2 * deltaH0f (SO3) - 2 * deltaH0f(SO2) - deltaH0f(O2)

deltaH0r = 2 ( - 395.7 ) - 2 ( - 296.8 ) - 0

deltaH0r = - 197.8 kJ for the conversion of 2 mol of SO2 to 2 mol of SO3

Assuming ideal gas equation,

P V = n R T

1.00 * 1.12 = n * 0.0821 * 298.15

n = 1.00 * 1.12 / (0.0821 * 298.15)

n = 0.0458 mol

For the conversion of 2 mol of SO2 to 2 mol of SO3, deltaH0r = - 197.8 kJ

Then,

for the conversion of 0.0458 mol of SO2 to 0.0458 mol of SO3, deltaH0r = 0.0458 * (-197.8) / 2 = - 4.53 kJ

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

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