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Posted by on Tuesday, April 3, 2007 at 10:07pm.


H2 +CO2-->H2O + CO
When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.
[H2]= 0.20mol/L
[CO2]= 0.30mol/L
[H2O]=[CO]= 0.55mol/L

a/ what is the mole fraction of CO in the equilibrium mixture?
b/ using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constanst for the reaction.
c/ determine Kp in terms of Kc for this system.
d/ when the system is colld rom 2,000K to a lower temperature, 30.0 percent of the CO is converted back to CO2. Calculate the valu of Kc at this lower temperature.
e/in a different experiment, 0.50mole of H2 is mixed with 0.50 mole of CO2 in a 3.0-liter reaction vessel at 2,000K. Calculate the equilibrium concentration, in moles per liter, of CO at this temperature.

You may be confused but surely you know how to do parts of this? Tell me what you don't understand about it and I can help you through it. For starters, the mole fraction of CO = mols CO/total mols.

  • AP CHEM! - , Wednesday, April 2, 2008 at 1:07pm


  • AP CHEM! - , Wednesday, April 2, 2008 at 1:07pm


    we're doing this in class right now.... :/

  • alfuz kaxhbo - , Monday, February 9, 2009 at 1:01am

    cpezdihl akjyvgrm skxeucna ezsdpgwft dcza yoxamue fqhjpse

  • AP CHEM! - , Sunday, April 12, 2009 at 8:00pm

    Behold my glory!

  • AP CHEM! - , Tuesday, April 28, 2009 at 7:38pm

    Can someone please answer this

  • AP CHEM! - , Tuesday, April 28, 2009 at 7:43pm

    How do you do D & E

  • AP CHEM! - , Monday, March 1, 2010 at 9:38pm

    I'm not so sure about E, but if you do the ICE chart, and equate Kc to 5, you can solve by plugging in the values of your Equilibrium concentrations into your Kc equation(again, refer to b). My answer is 0.118M CO, but I could be wrong.

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