Final answer:
To find the equilibrium masses of compounds after changing the container volume, calculate moles from the initial mass and volume, then adjust concentrations for the new volume. Use the molar mass to convert back to grams. Assumptions include constant temperature and no phase changes or reactions besides the one described.
Step-by-step explanation:
Solving for Equilibrium Concentrations and Masses
To calculate the final amounts of compounds present at equilibrium when the volume of the container changes, we must consider the conservation of moles and the fact that equilibrium constants are independent of the volume of the container.
Using the initial masses given for SbCl₅, SbCl₃, and Cl₂ in a 5.00-L container at equilibrium, we first convert these masses to moles using their molecular weights, then to molarity by dividing the moles by the volume of the container. For a new volume, the number of moles remains constant but the molarity changes. Since the ratio of the molar concentrations at equilibrium will still respect the equilibrium constant, we can use this to find the new molarities and from them, calculate the new masses of each compound.
Let's take an example calculation for SbCl₅ (molar mass roughly 299.0 g/mol). The initial moles are:
In a 2.00-L container, the concentration of SbCl₅ becomes (0.01287 mol / 2.00 L) = 0.006435 M, and the mass is (0.006435 M * 2.00 L) * 299.0 g/mol = 3.85 g.
However, note that this calculation assumes no change in temperature and that the main effect of volume change is on concentration, affecting the positions of equilibrium according to Le Chatelier's principle. It also disregards any potential phase changes or chemical reactions that might occur upon compression.