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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: defang01 on June 21, 2005, 11:09:54 AM

Title: HeLp: Equlibrium/Concentration
Post by: defang01 on June 21, 2005, 11:09:54 AM

Here is the question:

The equilibrium constant for the reaction 2BrCl (g) = Br2 (g) + Cl2 (g) is 32 at 500 K. A mixture of BrCl, Br2 and Cl2 each at 0.050 M, was introduced into a container at 500 K. Which of following is true?

The answer is B) the system is at equilibrium and therefore no net change occurs.  

But I think D) The reaction proceeds to the right, forming more products   is correct.

Shouldn't the reaction proceed until (Br2)x(Cl2) / (BrCl)^2 equals to 32, which means the reaction will proceed to the right?  

Can anyone tell me which choice is correct?

THANKS

Title: Re:HeLp: Equlibrium/Concentration
Post by: Demotivator on June 21, 2005, 03:28:04 PM

You're right. D.