[tiny]

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A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00-L vessel at 700 K??/ help???
A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00-L vessel at 700 K. These substances react as follows:

H2(g) + Br2(g) <==> 2 HBr(g)

At equilibrium the vessel is found to contain 0.566 g of H2.


a) Calculate the equilibrium concentrations of H2, Br2, and HBr.
b) Calculate Kp?


thanks soo much...

[Astrokel]

hey tiny!

show your attempts so we could help you in the parts which you don't understand. 

Do you know the relationship between Kp and Kc?

[tiny]

ok..yeah i do ..i know that Kp = Kc (RT) raised to delta N...or that its C^c *D^d/ A^a * B^b..

What i did i found the mols of  h2( .6815) and Br(.440)..but i cant seem to find the mols of HBr..thats the part thats given me trouble...can u help me with that please...,

[Astrokel]

hey,

draw up an ice table, you have the mass of H2 at equilibrium, so its easy to fill up the table.

the amount of Br2 you have calculated is at the initial and not at the equilibrium.