Changes in pressure can have a large effect on equilibrium systems containing gaseous components. 1. changing the concentration of gaseous components 2. adding an inert gas has no effect since the gas does not take part in the reaction, all partial pressures stay the same 3. changing the volume of the reaction vessel. This will cause a shift in the equilibrium position if the number of moles of gas is different on the reactant and product side (so LaTeX: / Delta Δ n = n products - n reactants) How would you change the volume for each of the following reactions to increase the yield of the product (s) ? 1. CaCO3 (s) ⇋ CaO (s) + CO2 (g) 2. S (s) + 3F2 (g) ⇋ SF6 (g) 3. Cl2 (g) + I2 (g) ⇋ 2ICl (g)

Equation 1: Increase the volume

Equation 2: Decrease the volume

Equiation 3: There is no effect in changing the volume

Explanation:

Equiation 1: When the volume is increased, the concentration of CO2 (g) is decreased, and the equilibrium will shift to increase the concentration change.

Equiation 2: Decreasing the volume of an equilibrium system will shift the reaction system towards the side in which there are less moles of the gas to matain the equilibirum constant. As there are less moles of gas in the products than in the reactants the equilibrium will increase the yield of the products.

Equation 3: There are the same amount of moles of gas in the equilibrium system (1 mole of each two reactans and 2 moles of the product), changing the volume will have no effect in the reaction, so the yield of the products will not be changed.