Posted by Student on Friday, February 24, 2012 at 10:15pm.
I don't know how to do this question, I understand we have to use ICE but I keep getting the wrong answer when I solve for x, it's just not working for me.
Consider the following reaction:
A(g) > 2B (g)
Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm . Make any appropriate simplifying assumptions.
1. Kp = 1.6
2. Kp = 1.4*10^4
3. Kp = 1.6*10^5

Chemistry Help PLEASE!!  DrBob222, Friday, February 24, 2012 at 10:21pm
Why don't you show me what you've done for #1 and I can see what the problem is.

Chemistry Help PLEASE!!  Student, Friday, February 24, 2012 at 10:45pm
I think I realized what my mistake was, I assumed the reaction would go to the right, doesn't it go to the left?

Chemistry Help PLEASE!!  DrBob222, Friday, February 24, 2012 at 10:59pm
Yes, it must go to left when you have started with zero A and have only B present.

Chemistry Help PLEASE!!  Student, Saturday, February 25, 2012 at 12:19am
Got it! Thank you :)
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