The burning of fuels with sulfur content produces sulfur dioxide (SO2) that can be oxidized to sulfur trioxide (SO3) and when reacting with rainwater gives rise to sulfuric acid and thus the phenomenon known as acid rain occurs. according to the reactions: 2S (g) + 2O2 (g) → 2SO2 (g)

2SO2 (g) + O2 (g) → 2SO3 (g)

SO3 (g) + H2O (l) → H2SO4 (aq)

The overall reaction is as follows:

2S (g) + 3 O2 (g) + H2O (l) → H2SO4 (aq) + SO3 (s)

Suppose that this reaction is to be carried out at 298K in a closed 1.0 liter container into which 0.75 mol of S (g), 0.4 mol of O2 and 1 mol of water are to be injected and that at a particular moment during reaction, molecular oxygen is reacting at the rate of 0.024 M / s.

After equilibrium was established, it was found that 0.0931 mol of H2SO4 had been formed, and that 0.57 mol of S2 (g), 0.1207 mol of O2 (g) and 0.9069 mol of H2O (l) remained unreacted.

The enthalpy of formation values ​​are as follows:

Substance ΔH ° f (kJ / mol)

S (g) 278.81

H2O (l) -285.83

O2 (g) 0

H2SO4 (aq) -909.27

SO3 (g) -395.72

Develop a report that contains the following:

1. The balanced reaction.

2. Amount in grams of the products and reactants that are formed.

3. Determine what the limiting reactant is

4. Volume of sulfuric acid produced and its concentration in units of molarity and normality.

5. If that volume of sulfuric acid is actually obtained, what is the yield (%) and selectivity (%) of the chemical reaction?

6. The equilibrium constant of the reaction.

7. The rate at which sulfuric acid is formed and at which S (g) reacts.

8. The energy required for the reaction to take place.

9. Analysis of results.