What are the partial pressures of H2, Br2, and HBr at equilibrium?

[mike1967]

Homework Statement

at 1000K, Kp=1.2*10^6 and Delta H = -101.7 kJ for the reaction H2(g)+ Br2(g) <-->2HBr.

A 0.952 mol quantity of Br2 is added to a 1.00L reaction vessel that contains 1.25 mol of H2 gas at 1000K . What are the partial pressures of H2 ,Br2 ,HBr and at equilibrium?

Homework Equations

PV=nRT
Kc=Kp(RT)^n
Kc=products over reactants reased to power of stoichiometric coefficients

The Attempt at a Solution

P=nRT/v
Pi(H2)=(1.25)(.08206)(1000)=78.121
Pi(Br2)=(.952)(.08206)(1000)=102.575

2.1*10^6=((2x)^2)/(78.121-x)(102.575-x))

x=78.121

Pf(H2)=102.575-x=25.45
Pf(Br2)=78.121-x=0
Pf(HBr2)=2x=156.24

Mastering Chemistry rejected

 

[Borek]

I just skimmed so it is possible I missed something, but at first sight nothing cries "wrong!", apart from the significant digits in the final answer.

I wonder why they give delta H? It is not clear if the final temperature is still 1000K.

 

[mike1967]

It ends up they wanted
Pf(H2) as 24.5
Pf(Br2) as 4.75*10^-4
Pf(HBr) as 156