posted by Katie .
The reaction is Br2 (g) <---> 2Br (g).
It occurs at T = 1600 C.
When 1.05 mol Br2 are placed in a 2 Liter flask, 2.50% of Br2 undergoes dissociation. Calculate the Kp for the reaction.
Okay so i did the ICE table for this,
Br2 (g) <---> 2Br (g)
I : 1.05/2 ..... 0
C : -x ......... 2x
E : (1.05/2) - x .... 2x
But I don't know what to do next..
Please help and thank you in advance.
Where did the 1.05/2 come from? Does that reflect the 2.5%? If so shouldn't it be 1.05*0.025 = 0.02625?
......Br2(g) ==> 2Br(g)
The E line uses mols; use PV = nRT to calculate p, the substitute into Kp expression and solve for Kp.
I've used too many significant figures so you need to go through the estimates I've made with that in mind.