Question
Asked Feb 13, 2020
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For a system, H2(g) + I2(g) ⇌ 2 HI(g), Kc = 62.9 at 750 K. 2.80 moles of HI were placed in a 10.0-liter container, brought up to 750 K, and allowed to come to equilibrium. Which situation described below is true, at equilibrium?

a. [HI] = 2 × [H2] b. [HI] = [H2] c. [HI] < [H2] d. [HI] > [H2] e. [H2] > [I2]

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Expert Answer

Step 1

The reverse reaction can be written as shown below.

Chemistry homework question answer, step 1, image 1

The expression for equilibrium constant for the above reaction can be written as shown below,

Chemistry homework question answer, step 1, image 2

Step 2

Given that, the initial number of moles of HI is 2.80 mol. The volume of the container is 10.0 L. The initial concentration of HI can be calculated as given below.

Chemistry homework question answer, step 2, image 1

An equilibrium table can be set up as given below.

Chemistry homework question answer, step 2, image 2

Now, these values in the fourth row can be inserted in the equilibrium constant expression as shown below.

Chemistry homework question answer, step 2, image 3

Now, the above equilibrium expression can be solved for

Chemistry homework question answer, step 2, image 4

...

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