Consider the gas-phase reaction, Cl2(g) + Br2(g) <=> 2 BrCl(g), for which Kp = 32 at 500 K. If the mixture is analyzed and found to contain 0.8 bar of Cl2, 0.6 bar of Br2 and 3.9 bar of BrCl, describe the situation:
Correct description:
Q < K and more products will be made to reach equilibrium.
How does that make sense!? Shouldn't it proceed in the reverse direction, since there is an excess of products?
2007-02-28 09:15:29 · 2 answers · asked by other_user 2 in Science & Mathematics ➔ Chemistry
It makes perfect sense. It doesn´t matter if you have more products, the equilibrium pressures must follow the equation BrCl square / Cl2*Br2. In the initial conditions Q=31.6 and K is 32, so BrCl should be higher and Cl2 and Br2 lower so that K=Q=32.
2007-02-28 09:26:45 · answer #1 · answered by ger 3 · 0⤊ 0⤋
The concentration of products divided by the product of the concentrations of reactants is less that 32. You have to look at where the situation is relative to the equilibrium constant. Things aren't all going to a point where they're equal, and the equilibrium constant describes what the ratios of reactants to products will be once the situation reaches equilibirum. In this case, since Kp is higher than the current situation, that means you are displaced from equilibrium in the direction of excess reactants.
2007-02-28 09:24:58 · answer #2 · answered by Professor Beatz 6 · 0⤊ 0⤋