Homework Help: chemistry

Posted by Mima on Saturday, April 7, 2012 at 6:15pm.

carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constanst (K) for this reaction (delta Gf values: H2CO3= - 616.1, H2O= - 237.1, CO2= - 394.4) .

Carbonic acid then ionizes in water (Ka1= 4.5 x 10^-7). Ignoring Ka2, estimate (K) for the overall process by which CO2 and H2O form H and HCO3.

What is the pressure of CO2 in equilibrium with carbonated water at 25 C and PH= 4.78?

chemistry - DrBob222, Saturday, April 7, 2012 at 10:28pm
CO2 + H2O ==> H2CO3
dGrxn = (dG products) - (dG reactants)
Then dG = -RTlnK
Solve for K.

Then H2CO3 ==> H^+ + HCO3^-
k1 = 4.5E-7
For the two reactions together you have
CO2 + H2O ==>H^+ + HCO3^- and Keq = k1K.

Finally, convert pH 4.78 to H^+, substitute into the equation (HCO3^- = H^+ too) and solve for partial pressure of CO2.
chemistry - Mima, Sunday, April 8, 2012 at 12:03am
Thank you so much for replying, but I can't understand how to solve for partial pressure of CO2, when I get the [H^+] from PH then how to solve for partial pressure of CO2?
chemistry - Mima, Monday, April 9, 2012 at 1:45pm
Thanks a lot, I got it.
chemistry - Amanda B., Sunday, April 14, 2013 at 6:27pm
I kept record of all IP addresses and they will be reported to UCI undergrad offices.
chemistry - Dude, Wednesday, April 17, 2013 at 11:00pm
@Amanda lolololol
chemistry - John, Wednesday, April 17, 2013 at 11:01pm
@Amanda, k

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