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Problem with the ICE TABLE
the rael walter white:
For the reaction 2HI -> H2 + I2 (all gas phase) the value of the equilibrium constant at 700K is 0.0183. If 3.0 moles of HI are placed in a 5-liter vessel and allowed to decompose according to the above equation, what percentage of the original HI would remain at equilibrium
Can someone explain why the equilibrium concentration constant for 2HI IS .6-X AND NOT .6-2X when filling out the ice table
Borek:
Can you show complete ICE table for this problem? A lot depends on what x refers to.
Orcio_87:
Initial concentration of HI is 0,6 mol / liter, so final concentrations of HI, H2 and I2 are 0,6 - x, 1/2 x and 1/2 x (two molecules of HI produces only one H2 and one I2).
Borek:
--- Quote from: Orcio_Dojek on September 12, 2021, 07:29:39 AM ---Initial concentration of HI is 0,6 mol / liter, so final concentrations of HI, H2 and I2 are 0,6 - x, 1/2 x and 1/2 x (two molecules of HI produces only one H2 and one I2).
--- End quote ---
Or 0.6-2x, x and x, depending on what the x is. Both approaches are OK, it is just about knowing which one you use and what you solve for.
the rael walter white:
I totally agree but the solution we were given below confuses the heck out of me
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