# P1 Equilibrium question

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0.50 mol of I2(g) and 0.50 mol of Br2(g) are placed in a closed flask. The following equilibrium is established.

I2(g) + Br2(g)  IBr(g)

The equilibrium mixture contains 0.80 mol of IBr(g). What is the value of Kc?

Should I change the mol into mol dm-3?

Thank you.

Edited by allthebest

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Hints:
1) Balance the equation
2) Assume a variable V for volume of container and calculate concentration using V.
3) What are the concentration of reactants at equilibrium? (Why do you need this?)
Plug into definition of equilibrium constant and simplify!
PM me if you are still stuck.

Edited by kw0573

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2 hours ago, kw0573 said:

In the interest of providing you an answer. You should give us the COMPLETE question. You didn't even give ANY question. When you update the question I'll update this answer.

Sorry, I forgot to put the question. I've updated now. Thanks

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0.8 mol of IBr reacts with 0.4 mol of I2 and Br2 (because of the 2:1 ratio). So the equilibrium mixture has 0.8 mol of IBr and 0.1 mol of I2 and Br2.

Write the equilibrium expression, plug in those equilibrium values and you'll get 64 (0.64/0.01).

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