Question

Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I₂(g)+Cl₂(g)?2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.35atm and PCI₂=0.35atm .What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?

Answer 1

To determine the partial pressure of iodine monochloride (ICl) at equilibrium, we can use the reaction's equilibrium constant (Kp) and the initial pressures of the reactants.

Step-by-step explanation:

To determine the partial pressure of iodine monochloride (ICl) at equilibrium, we can use the reaction's equilibrium constant (Kp) and the initial pressures of the reactants. According to the balanced chemical equation, the stoichiometric coefficient for ICl is 2.

First, we need to calculate the initial pressure of ICl. Since we have equal initial pressures of I2 and Cl2, the initial pressure of each reactant is 0.35 atm.

Using the equilibrium constant expression, Kp = [ICl]^2 / ([I2] * [Cl2]), we plug in the given values and solve for [ICl].