[Shaun1979]

Given [H2] = 0.0343 M, [I2] = 0.326 M, and [HI] = 0.826 M for the following
reaction at 440oC. Calculate the equilibrium constant.
I2 (g) + H2 (g) → HI (g)


I am trying to complete this question as part of revision for up and coming exams.

Is the answer:

[0.826]2/ [0.0343][0.326] = Kc = 61.017 (at 440oC)

correct?

[LoveInQuanta]

Hey Hey, Shaun,

is the coefficient of HI in the equation actually 2, and you just failed to type it in? If so, your equation is correct, and if not, then you should remove the squaring of the [HI] in the numerator.

Your math is right, if indeed the equation is

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

[Shaun1979]

Thanks for your reply.

I thought that in order to balance the equation, I would need to add the coeficient 2?

Hmmmmmm, by not placing the coefficient there, how can the equation be in a state of equilibrium?

[LoveInQuanta]

You do need to add the coefficient 2. But you just didn't type it, so I was making sure that that's what you meant

[Shaun1979]

Sorry, chemistry confuses me at the best of times!

That is how they asked the question (without squaring HI), and then I went ahead and squared it when doing Kc, in order to balance it (otherwise it makes no sense).

So I am assuming that I was right in doing so, and that's what you mean?