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) .

Question

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?

Answer 1

@Amanda lolololol

Answer 2

@Amanda, k

Answer 3

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?

Answer 4

Thanks a lot, I got it.

Answer 5

I still don't understand how to find the partial pressure of CO2. I've got the H+ concentration but I'm stuck at that step.

Answer 6

the partial pressure is determine by

K= [hc03][h]/pressure

Answer 7

So the pressure =.202 atm

Answer 8

where do you get the T in the first one?

Answer 9

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) .

@Amanda lolololol

@Amanda, k

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?

Thanks a lot, I got it.

Thanks!

I still don't understand how to find the partial pressure of CO2. I've got the H+ concentration but I'm stuck at that step.

the partial pressure is determine by

So the pressure =.202 atm

where do you get the T in the first one?

I don't understand how to find the partial pressure can someone explain it to me please I have a homework due tonight that is similar to this