Asked by linds
IM SO CONFUSED PLEASE HELP!
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.
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.
Answers
Answered by
Ahmad
ROFL YOU'RE STUPID
we're doing this in class right now.... :/
we're doing this in class right now.... :/
Answered by
alfuz kaxhbo
cpezdihl akjyvgrm skxeucna ezsdpgwft dcza yoxamue fqhjpse
Answered by
God
Behold my glory!
Answered by
Dazed and confused
Can someone please answer this
Answered by
Dazed and confused
How do you do D & E
Answered by
Not Sure
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.
There are no AI answers yet. The ability to request AI answers is coming soon!