Problem: Diatomic iodine (I2) decomposes at high temperature to form I atoms according to the reaction: I2(g) ⇌ 2I(g), Kc = 0.011 at 1200 oCIn an equilibrium mixture, the concentration of I2 is 0.18 M. What is the equilibrium concentration of I?

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Kc = productreactantKc = [I]2[I2][I]2 =Kc[I2][I] =Kc[I2]


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Problem Details

Diatomic iodine (I2) decomposes at high temperature to form I atoms according to the reaction: I2(g) ⇌ 2I(g), Kc = 0.011 at 1200 oC

In an equilibrium mixture, the concentration of I2 is 0.18 M. What is the equilibrium concentration of I?

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Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.

What professor is this problem relevant for?

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