Partial pressure of reagent in reaction

[Denver Dang]

1. The problem statement, all variables and given/known data
I have the reaction:

A(g) + 2B2(g) -> AB4(g)

The equilibrium constant K(T=298) = 10, and all gases are ideal.

So the two reagents A and B are mixed together at 1 bar and T = 298K, with the quantities 1 mol of A and 1 mol of B.

Now I have to find the partial pressure of AB4 when there is equilibrium in the reaction.


2. Relevant equations

?


3. The attempt at a solution
I've looked at Dalton's Law, but nothing I did seemed to make sense. So I'm kinda stuck.

I know the result should be: 0,268 bar.

So, could anyone give me a hint ?


Thanks in advance.

Regards.

[Borek]

Have you tried ICE table approach?

This is not very difficult - you have to calculate amounts of substances at equilibrium. Write expression for K and think how concentrations of all substances change during the reaction - they are linked by stoichiometry.

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