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Can any one help me solve this chemistry problem?

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In the reaction below, 8.97 atm each of Cl2 and I2 were placed into a 1.00 L flask and allowed to react:

Cl2(g) + I2(g) <=> 2 ICl(g)

Given that Kc = 53.2, calculate the equilibrium pressure of Cl2

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  1. Let &quot;x&quot; be the pressure loss due to rxn of either Cl2 or I2.  

    Then,  (2x)^2/(8.97-x)^2  = 53.2

    x is about 7 atm, so desired pressure is about 1.97 atm.

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