Problem: 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 = 0.35 atm and PCl2 = 0.35 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?

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FREE Expert Solution
FREE Expert Solution

We’re given the following equilibrium reaction:

I2(g) + Cl2(g)  2 ICl(g); Kp = 81.9 (at 298 K)


We know that the initial pressure of I2 and Cl2 is 0.35 atm. From this, we can construct an ICE table:



The Kp expression for the reaction is:



Note that each pressure is raised by the stoichiometric coefficient: PI2 and PCl2 is raised to 1 while PICl is raised to 2. Plugging in the equilibrium pressures from the ICE table into the Kp expression:


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Problem Details

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 = 0.35 atm and PCl2 = 0.35 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?

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Based on our data, we think this problem is relevant for Professor Houston's class at CSUS.