Final answer:
The question is about calculating the equilibrium constant Kp for the reaction of PCl₅ decomposition based on the initial moles, final total pressure, temperature and the gas constant without providing specific reaction details or changes in the number of moles.
Step-by-step explanation:
The question involves calculating the equilibrium constant (Kp) for the decomposition of PCl₅ at a certain temperature and volume, given the initial moles of PCl₅ and Argon, the final total pressure, temperature, and the universal gas constant R.
First, we would set up the equilibrium expression for the decomposition of PCl₅ into PCl₃ and Cl₂, and then use the given total pressure at equilibrium to determine the partial pressures of each component. We would apply the ideal gas law to relate moles, volume, temperature, and pressure.
This allows us to find the individual partial pressures of PCl₃ and Cl₂ from the dissociation of PCl₅. Using these partial pressures, we can calculate Kp. It's essentially about applying the principles of chemical equilibrium and the laws of gases to find the constant.
However, as there are some missing values or steps in the data provided, we cannot complete the calculation. Typically, we would calculate the change in moles due to the reaction, translate this into partial pressures using the ideal gas law, and then substitute these into the formula for Kp.