Jarred Awesome

Hello Everyone, I’m by no means a chemist, but I have been trying to learn a little bit about it, for a project I’m working on. I don’t know where else to ask, so I figured this forum might be a good place. I have an aquarium, and I am trying to calculate how much co2 is dissolved in the tank. If I understand properly, I can permanently put an upside down cup in the water, and use Henry’s Law to figure this out. Attached you can find a drawing of my set up. I can also use Antoine’s equation compensate for temperature Here is what I came up with, but I don’t have enough knowledge to know if I’m doing this properly can someone see if I am doing this properly? I took the temp of water, the applied Antoine Equation to get the Vapour Pressure in the cup. (Not sure if that’s what I am supposed to do) I then took the PPM measured in the cup, and the result from the Antoines equation And applied it to this: PA=(ppm/PV)x10e6, in order to get the partial pressure. I then applied the result into Henry’s law to get the result in M/L, Then multiplied it by 44010 to get the readily as ppm Here is the raw math. co2 in cup = 195PPM Water temp in aquarium = 27 C Antoine Equation(with constants from water put in): 10^(a-b/(T+c)) 10^(7.94917-1657.462/(27+227.02) =19.887130064 mmHg Ppm to Partial Pressure Partial Pressure = PPM/10^6*Vapor Pressure (195/10^6)*19.887130064 =0.039687554121637006 mmHg Then Henry’s law kh = 29.95 c = pa/kh ppm = c*44010 Dissolved gas = Partial Pressure / Henry's constant 039687554121637006 / 29.95 =000129907122206828293 M/L Then converting m/L into ppm mmHg * Mollar Mass of given Gas 000129907122206828293 * 44010 Rounded that gives me 5.71ppm if co2 in the aquarium. My hope is someone can tell me if my my math and implantation is correct?