Question

Consider the following system at equilibrium where Kc = 34.5 and H° = -198 kJ/mol at 1150 K. 2 SO2 (g) + O2 (g) -->2 SO3 (g) The production of SO3 (g) is favored by: Indicate True (T) or False (F) for each of the following:

1. increasing the temperature.

2. increasing the pressure (by changing the volume).

3. increasing the volume.

4. removing SO3 .

5. removing O2 .

Answer 1

Given, the balanced equilibrium reaction,

2SO₂(g) + O₂(g) 2SO₃(g) -----H= -198 kJ/mol

The production of SO₃(g) is favored by,

1) Decreasing the temperature, since the reaction is exothermic.

2) Removing SO₃(g) since the equilibrium will shift to the product side.

3) Increasing the concentration of reactants.

4) Increasing the pressure Or decreasing the volume, since, the reaction goes to that direction where the fewer the number of gaseous molecules. (In the given reaction product side has a fewer number of gaseous moles)

Thus,

1) Increasing the temperature ---- False

2) Increasing the pressure(Decreasing the volume) --------True

3) Increasing the volume -------- False

4) Removing SO₃ -------- True

5) Removing O₂ ---------- False