1. Find the equlibrium constant if there is 0.030moles/L of Carbon Dioxide going in the forward direction and water is in excess to form Carbonic Acid (H2CO3) 2. Relevant equations [products]/[reactants] = K 3. The attempt at a solution I'm trying to figure out how Carbon Dioxide in the atmosphere will affect the chemistry of the oceans. From my research I've found that CO2(g) = CO2(aq) in water is 1.45 g/L where I deduced a equilbrium of 0.030 moles/L. My next step is where I have to figure out how much Carbonic Acid is made (CO2 + H20 = H2CO3) when I know that the equlibrium for the forward direction is 0.039 L/mol. So: [H2CO3]/[CO2][H2O] which based on what I know translates to [H2CO3]/(0.03)[[H2O] = 0.039L/mol However, L/mol is not the same as mol/L and I need to find the concentration of [H2CO3] because after that I need to figure out the K values for H2CO3 = H++HCO3 and HCO3 = H++CO3 equilibriums *sorry, I do apologize but I'm not sure how to get the "reversible reaction" symbol on the physics forums, so I just used an "=" sign * ps. I was read on wikipedia that the solubility of Carbon Dioxide is 1.45g/L at 25 degrees C at 100kpa. The pressure, is that including the rest of the atmosphere? or just the carbon dioxide alone? because I've calculate the partial pressure of the CO2to be 11.6139 pa at sea level.