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A. Writethebalancedequationforthehalfreactionthattakesplaceatthecathode(theelectrode where H2 is produced) during the electrolysis process. 2H2O (l)+2e− →H2 (g)+2OH− (aq) B. Calculatetheamountofelectricchargeincoulombs(C)thatpassesthroughthesolutioninone of the electrolytic cells in the OGS in a 24-hour period. 50. amp = 50. C s (See Figure 2.) According to the balanced equation, when water decomposes, twice as many moles of hydrogen are produced than the amount of oxygen. 2 H2O (l) → O2 (g) + 2 H2 (g) D. CalculatethenumberofmolesofO2(g)producedinonecellduringthe24-hourelectrolysis period. The half reaction that takes place at the anode: 2H2O (l)→O2 (g)+4H+ +4e− molO =4.3×106 C⋅ 1mole− ⋅1molO2(g)=11molO (g) 2 99.65×105 C 4mole− 2 E. Calculate the volume of O2 in liters (L) produced in one cell during the 24-hour electrolysis period at 298 K and 1 atm of dry O2(g). 50.C 60s 60min 6 ⋅ 24h=r 4.3×10 C C. WhyisthevolumeofH2(g)collecteddifferentfromthevolumeofO2(g)collected? ElectricCharge= ⋅ ⋅ 1s 1min 1hr V = nRT P VO = 2 (11molO )⋅0.0821Latm⋅(298K) 2 mol K 1atm =270LO2 F. Based on the information provided, how many electrolytic cells would be needed in the OGS to produce enough O2 to support a crew of six astronauts? How much O2 (in liters) needs to be generated for a 12-day mission if each astronaut consumes 0.91 kg of O2 per day? 6crew⋅0.91kgO2 ⋅1000g⋅ 1molO2 =170molO2 crew 1 kg 32.02 g O2 Use the answers found in questions D: 170 mol O2 ⋅ 1 cell =15 cells 11 mol O2 Use the answers found in questions E: 15 cells ⋅ 270 L O2 ⋅12 days = 4.9 ×104 L O2 cell ⋅ day www.nasa.gov Oxygen Generator System 4/5PDF Image | OXYGEN GENERATOR SYSTEM
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