Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: the rael walter white on September 12, 2021, 01:15:39 AM
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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
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Can you show complete ICE table for this problem? A lot depends on what x refers to.
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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).
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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).
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.
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I totally agree but the solution we were given below confuses the heck out of me
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Do you guys think this guy is right or am I just completely lost
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Do you guys think this guy is right or am I just completely lost
No, this solution is incorrect and you are perfectly right being confused. Stoichiometric coefficient of 2 is missing (either as just "2" or as "1/2").