Final answer:
To calculate the equilibrium concentration of Cl2 in a 1.00-liter vessel containing PCls and PC13, you can use the equilibrium constant (Kc) and the initial concentrations. With an ICE table and the given equation Kc = (E(Cl2))/(E(PCls) * E(PC13)), you can solve for the unknown change in concentration (C(Cl2)) using the formula (2.24 x 10^2) = E(Cl2)/((0.235 - C) * (0.174 - C)). From C(Cl2), you can then determine E(Cl2) and the equilibrium concentration of Cl2 in moles per liter.
Step-by-step explanation:
To calculate the equilibrium concentration of Cl2 in a 1.00-liter vessel, we can use the given equilibrium constant (Kc) and the initial concentrations of PCls and PC13. Firstly, we need to set up an ICE table, where I represents the initial concentration, C represents the change in concentration, and E represents the equilibrium concentration. PCls has an initial concentration of 0.235 mol and PC13 has an initial concentration of 0.174 mol. Since Cl2 is a product of the reaction and its stoichiometric coefficient is 1, we can assume its initial concentration is 0. To find the equilibrium concentration of Cl2, we can apply the formula: E(Cl2) = I(Cl2) + C(Cl2). From the ICE table, it can be determined that C(Cl2) is equal to the change in concentration of PCls or PC13, which is unknown. To solve for C(Cl2), we need to calculate the value of the equilibrium constant. Kc is equal to the concentration of Cl2 over the product of PCls and PC13. Given that Kc is 2.24 x 10^2, we have the equation Kc = (E(Cl2))/(E(PCls) * E(PC13)). Substituting the given values into the equation, we have (2.24 x 10^2) = E(Cl2)/((0.235 - C) * (0.174 - C)). Solving this equation will give us the value of C and subsequently E(Cl2). Once we have E(Cl2), we can get the equilibrium concentration of Cl2 in moles per liter.