Consider the following chemical reaction H_2 (g)(I_2 (g) 2 2 HI (g) Sherman plac

Question

Consider the following chemical reaction H_2 (g)(I_2 (g) 2 2 HI (g) Sherman placed 0.0218 moles of H_2 gas and 0.145 moles of I_2 gas and 0.0783 moles of HI gas into a 3.50 liter flask at 430.0 degree C. Dudley noted that the KC for this reaction at 430.0 degree C was 54.3. Mr. Peabody has asked Sherman and Dudley to answer the following questions: Given the above experimental conditions, is the above reaction at equilibrium? Show work! If it is not at equilibrium, what is the direction the reaction would shift to obtain equilibrium?

Explanation / Answer

    H2(g) + I2(g) -------------> 2HI(g)

     Qc = [HI]2/[H2][I2]

            = (0.0783)2/0.0218*0.145

            = 1.94

Kc     = 54.3

Qc not equal to Kc . So it is not equilibrium .

Kc> Qc the equilibrium shift to right side.

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