If co2 is being produced in the solution at a faster rate than h2co3 is the rate of the forward or reverse reaction faster?

Answer 1

Not sure why the carbonic anhydrase reaction was assumed, but I would look at this question in a different way. I would think the reaction in question is the following:

H2CO3 <==> H2O + CO2

If this reaction is at equilibrium, and the concentration of CO2 were to decrease, the reaction would shift to the right (product side) and the concentration of H2CO3 would decrease. This is because of Le Chatelier's principle whereby the system will shift in order to undo any perturbation that occurs at equilibrium, so as to try to restore the equilibrium.

Answer 2

It sounds like you're referring to the carbonic anhydrase equation, one of my favorites! Here is the full equation:

CO2 + H2O ⇔ H2CO3 ⇔ H+ + HCO3+

If the reaction moves forward, the products (H+ and HCO3+) is favored. If the reaction moves reverse, the reactants are favored (CO2 and H2O). The answer here is that the reverse reaction must be faster, leading to CO2 production. I hope this helps! Please let me know if you have any other questions!