Iodine chloride decomposes at high temperatures to iodine and chlorine gases. 2I

Question

Iodine chloride decomposes at high temperatures to iodine and chlorine gases. 2ICl(g) <--> I2(g) + Cl2(g) Equilibrium is established at a certain temperature when the partial pressures of ICl, I2, and Cl2 are (in atm) 0.43, 0.16, and 0.27, respectively a) calculate K? b)If enough iodine condenses to decrease its partial pressure to 0.10 atm, in which direction will the reaction proceed? What is the partial pressure of iodine when equilibrium is reestablished? Please show steps...thank you...:)

Explanation / Answer

a)2ICl(g) I2(g) + Cl2(g); kb=(0.16*0.27)/(0.43)^2; = 0.2336; b) in the backward direction c)give me the equlibrium presser :

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