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Anode Reaction Cathode Reaction ( 1/4moleO2 )(60sec) = 0.000155moleO2 (21) 96,487A-sec min A-min 1moleH+ 60sec moleH+ (96,487A-sec)( min ) = 0.000622 A-min (22) ( 1/2moleH2 )( 60sec) = 0.000311moleH2 (23) 96,487A-sec min A-min 1moleOH− 60sec moleOH− (96,487A-sec)( min ) = 0.000622 A-min (24) Therefore, seawater with a HCO3- concentration of 142 ppm (0.0023 M) and flow rate of 1 liter per minute, a theoretical applied current of 3.75 A will be required to lower the pH to less than 6.0 and convert HCO3- to H2CO3. 0.0023 mole HCO3− 1 Liter ( Liter )( min ) = 3.75A (25) 0.000622 mole H + ( A-min ) Current efficiency can be defined as the ratio of the theoretical minimum current predicted by Faraday's law to the actual current applied to the electrodes of the acidification cell. In actuality, current efficiencies are never 100 % and can range from 30 to 95 % based on the conductivity of the liquid being treated; the higher the conductivity, the greater the current efficiency. It is estimated that current efficiency for seawater is on the order of 70 to 90 %. Therefore, AcutalCurrent= (TheoreticalCurrent) = (3.75A) = 4.69A (26) Current Efficiency 80 % The theoretical amount of CO2 that can be removed from the acidified seawater is 0.0023 moles per liter. Removal efficiency can be defined as the ratio of the theoretical amount of CO2 removed to the actual amount of CO2 removed in the acidified seawater. Removal efficiencies are never 100 % and can range from 50 to 95 % based on various unit operating requirements. The overall removal of CO2 is conservatively estimated to be approximately 50 %. ActualRemoval=(TheoreticalRemoval)=(0.0023mole/min)= 0.0046 moleCO2 (27) Removal Efficiency 50 % min 10PDF Image | CO2 from Seawater
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