Final answer:
Determining the partial pressure of iodine monochloride (ICl) at equilibrium requires the complete chemical equation, initial pressures or concentrations, and the equilibrium constant at the reaction temperature. Without this information, the question cannot be answered fully. Typically, an ICE table is used to calculate equilibrium partial pressures or concentrations given the initial conditions and Kp or Kc.
Step-by-step explanation:
The partial pressure of iodine monochloride (ICl) when the reaction reaches equilibrium can be determined by using the equilibrium constant (Kp) for the reaction. However, the question as provided doesn't give enough information for a complete solution. We would need the complete chemical equation, the initial pressures or concentrations, and the value of Kp at the temperature of interest to answer this question. Typically, for a reaction given in the form A(g) + B(g) → C(g), the partial pressure of a substance at equilibrium can be found using the initial pressures, the change in pressures (x), and the equilibrium expression involving Kp.
To answer related questions regarding the equilibrium concentrations or partial pressures, we can refer to exercises provided, assuming they have similar missing data. For example, if considering the reaction H2(g) + I2(g) → 2HI(g) at equilibrium, with a provided equilibrium constant (Kc or Kp) value, and the initial concentrations or partial pressures of H2 and I2, we can use an ICE table (Initial, Change, Equilibrium) to solve for the equilibrium concentrations or partial pressures.