Question

Consider the following reaction: H2(g)+I2(g)⇌2HI(g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T(∘C) [H2] [I2] [HI] [Kc] 25 0.0355 0.0388 0.922 − 340 − 4.60×10−2M 0.394M 9.6 445 4.90×10−2M 4.76×10−2M − 50.2 Find Kc at 25∘C. Find [H2] at 340∘C. Find [HI] at 445∘C.

Answer 1

These are three questions.

Answer:

• Question 1) Find Kc at 25°C: 617

• Question 2) Find [H₂] at 340°C: 0.352 M

• Question 3) Find [HI] at 445°C: 0.342 M

Explanation:

I will start by copying the table for better understanding of the data and the work to do.

T(∘C)       [H2]                    [I2]                     [HI]               [Kc]

25           0.0355               0.0388              0.922            -

340                                    4.60×10⁻²M       0.394M         9.6

445         4.90×10−2M      4.76×10⁻²M           −                50.2

The chemical equation that represents the equilibrium is also given:

• H₂ (g) + I₂(g) ⇄ 2HI(g)

From that equilibrium equation, you can fnd the expression of the equlibrium constant, Kc, as:

$Kc=[HI]^2/([H_2][I_2])$

The calculations and explanations to answer the three questions are in the pdf file attached.

Please, click on the image of the file to open it.

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