Chapter 15, Problem 7SAQ

Consider the reaction between iodine gas and chlorine gas to form iodine monochloride.

   ${\text{I}}_{\text{2}}\left(\text{g}\right)+{\text{Cl}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons \text{2ICl}\left(\text{g}\right)$K_{p =} 81.9 (at 298K)

A reaction mixture at 298 K initially contains ${\text{P}}_{\text{I}}{}_{{}_{\text{2}}}=0.\text{25}$ atm and ${\text{P}}_{{\text{CI}}_{\text{2}}}=0.\text{25}$ atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?

• 2.3 atm
• 0.17 atm
• 0.41 atm
• 0.64 atm