Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: raiderhader2 on February 25, 2009, 08:44:15 PM
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achieved at 2000K
Following equilibrium concentrations:
[H2]=0.20 M
[CO2]=0.30 M
[H2O]=[CO]=0.55M
When the system is cooled from 2000K to a lower temperature, 30.0% of the CO(g) is converted back to CO2(g). Calculate the Kc at this lower temperature.
Here's what I tried:
[CO]=0.55M-(0.55M)(0.3)=0.39M
[H2O]=0.39M
[CO2]=0.30M+90.55M)(0.3)=0.47M
[H2]=0.20M+(0.55M)(0.3M)
Kc=(0.39M)^2/[(O.47M)(0.37M)]=0.87
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[H2O]=0.39M
Seems like you are on the right track, you just missed that water concentration must change as well.
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I think you have calculated right equilibrium concentrations.Your water concentration is also right.
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I think you have calculated right equilibrium concentrations.Your water concentration is also right.
Yep. I have misread the solution. My bad.