i am really stuck on a chemistry problem for ap?

A mixture of 1.374 g of H2 (subscript) and 70.1 g of Br2 (sub.) is heated in a 2.00 L vessel at 700 K. These substances react as follows: H2 (sub)(g) + Br2 (sub)(g) <> 2 HBr (sub)(g) At equilibrium the vessel is found to contain 0.566 g of H2 (sub). a. Calculate the equilibrium concentrations of H2 (sub), Br2 (sub), and HBr. b. Calculate Kc C. Calculate the equilibrium partial pressures of H2 (sub), Br2 (sub) and HBr. (hint-Pv=nRT, R=.0821L-atm /Mol K * sub means the number is a subscript i just dont know how to type it in internet explorer. <> is the arror sign used in this problem with to arrorws not facing each other. I believe it means at equilibrium. Also i usually don't ask school questions im just really stuck any help greatly appreciated. help!!!!!!!!!!!!!!!!!!!!!!!!

Asked By: guest987654321 - 3/7/2006
Best Answer - Chosen by Asker
i can help with part of it. i forgot a lot of my chemistry stuff. so ok first thing is to find the number of mols of each reactant put in. which is mass over molar mass. and then find the molar mass of 0.566g of H2. so you know how many moles of H2 are left over, so you should lknow how many moles reacted and you... More
Answered By: someguy - 3/13/2006
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