Problem: For the following reaction, if the initial concentration of PCl3 (g) is 1.0M and x is the equilibrium concentration of P4 (g), what is the expression for the equilibrium constant? PCl3 <--> P4 + Cl2
I balanced the equation... 4PCl3 <--> P4 + 6Cl2
In setting up my ICE box, I realize that the initial for P4 is 0, and that you would add "x" to get your equilibrium value...I still don't understand what to add/subtract for the other components of the reaction? Would I add 6x for Cl2 and subtract 4x from PCl3 because of the stoichiometric coefficients?
Thank you!
Quiz 3 Prep #7, setting up ICE box
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Re: Quiz 3 Prep #7, setting up ICE box
4PCl3 <---> P4 + 6Cl2
I: 1.0M 0 0
C: -4x +x +6x
E:1.0-4x +x +6x
the universal rule about ICE Box is that the ratios of "change" are the same as in the formula. Thus, the ratios: PCl3:P4:Cl2=4:1:6, are seen in the formula and the amount of change is the same.
I: 1.0M 0 0
C: -4x +x +6x
E:1.0-4x +x +6x
the universal rule about ICE Box is that the ratios of "change" are the same as in the formula. Thus, the ratios: PCl3:P4:Cl2=4:1:6, are seen in the formula and the amount of change is the same.
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Re: Quiz 3 Prep #7, setting up ICE box
The expression for the equilibrium constant would thus be:
(x)(6x)6 = Kp
(1-4x)4
Correct?
(x)(6x)6 = Kp
(1-4x)4
Correct?
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Re: Quiz 3 Prep #7, setting up ICE box
Kc I believe (talks about equilibrium concentration instead of equilibrium partial pressures)
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