Theoretically,
The potential difference that could be produced in a fuel cell operating with oxygen and hydrogen is 1.2 V but actually it is 0.5 to 0.6 V as the current flows.
However, here both the gases are at 5 bar therefore, the potential difference can drop to 0 V.
Self-test 5.4 What potential difference would be produced in a fuel cell operating with oxygen and...
Self-test 5.4 What potential difference would be produced in a fuel cell operating with oxygen and hydrogen with both gases at 5.0 bar?
Self-test 5.4 What potential difference would be produced in a fuel cell operating with oxygen and hydrogen with both gases at 5.0 bar? Consider the latimer diagram Cos* 1.92 Co2+ 20.282 Coo Fest 0.77 Fe²+ -0.44 Fe I write a balanced equation that occur between F2+, Fe and cost, Co2+ 2- Indicate whether any of the species on the - latimer diagram has a tendency to disproportionate.
In a hydrogen fuel cell, oxygen and hydrogen are combincd to produce water and a small potential differ- ence. The steps of the chemical reaction are: at-electrode: at + electrode: H2 + 20H-→ 2H2O + 2e-; O2 + H2O + 2e-→ 2OH-, Use the table of chemical values to calculate a) the work that can be produced from this fuel cell, b) the 'waste' heat produced during standard operation, c) the voltage of the cell, and d) the minimum voltage...
Hydrogen (H) and oxygen (O.) are reacted in a fuel cell to produce energy. The product of the reaction is water, and any excess gases are vented after the fuel cell, as shown in the figure below. The hydrogen and oxygen tanks are maintained at the same temperature and pressure, and they feed at the same volumetric flow rate. The reaction goes to 60% completion in the fuel cell (hydrogen basis) If all of the unreacted hydrogen and a portion...
Maximum Useful Work from a Fuel Cell. What is the maximum useful work which can be obtained from a hydrogen-oxygen fuel cell that produces 1.60 kg of water at 25°C? (Assume 1 atm pressure for the gases.)
1a. Suppose a hydrogen-oxygen fuel-cell generator was used to produce electricity for a house. Use the balanced redox reactions and the standard cell potential to predict the volume of hydrogen gas (at STP) required each month to generate the electricity needed for a typical house. Assume the home uses 1400 kWh of electricity per month. 1b. Suppose a hydrogen-oxygen fuel-cell generator was used to produce electricity for a house. Use the balanced redox reactions and the standard cell potential to...
1.3. How much gram of hydrogen is needed to operate a 50 kW hydrogen/oxygen fuel cell for 3 hours? The potential of the cell is 0.7 V (remember that Power-IV). Molecular weight of H2 is 2 g/mol. The reaction at the anode is H2 2H+ 2e
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Maximum Useful Work from a Fuel Cell. What is the maximum useful work which can be obtained from a hydrogen-oxygen fuel cell that produces 1.69 kg of water at 25°C? (Assume 1 atm pressure for the gases.)
Faraday’s Law 1. Hydrogen fuel cells are based on the reaction of hydrogen and oxygen to form water: 2H 2 (g) + O 2 (g) ? 2H 2O (l) In the presence of excess oxygen, a hydrogen fuel cell consumes 0.370 grams of hydrogen per hour at 25°C. Calculate the maximum current that can be produced by this fuel cell. 2. Aluminum is produced by the electrolytic reduction of alumina, Al 2O 3. The overall cell reaction can be written...
Hydrogen and oxygen gases are utilized as reactants for fuel cells. Hydrogen gas is oxid side to generate protons and electrons which move to the cathode side to react with oxygen to produce electricity and water as byproduct. Molecular weight: M(H2) -2 g/mol, M(O)-32 g/mol, M(H-0) - 18 g/mol. Detailed reactions in each side are described below: ized in the anode (-) side: | (+) side: Cell: H2 → 2H+ + 2e- E" 0.00V 202 + 2H+ + 2e-→ H2O...