Partial pressure of reagent in reaction

AI Thread Summary
To find the partial pressure of AB4 at equilibrium for the reaction A(g) + 2B2(g) -> AB4(g) with K(T=298) = 10, start by applying the ICE table method to determine the changes in concentrations of the reactants and products. Use Dalton's Law to relate the total pressure to the partial pressures of the components. The equilibrium expression for K must be set up based on the stoichiometry of the reaction. The final calculated partial pressure of AB4 should be 0.268 bar. Understanding the relationship between the concentrations and the equilibrium constant is key to solving the problem.
Denver Dang
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Homework Statement


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.

Homework Equations



?

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.
 
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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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