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:
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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