The thermodynamic data for the oxidation of one mole of hydrogen (hydrogen- oxygen fuel cell reaction)...
(1) About a hydrogen fuel cell, (a) The fuel is hydrogen. (b) There is an oxidation reaction on the surface of the anode. (c) The current flows from the anode to the cathode through the external circuit. (d) There is an oxidation on the surface of the cathode. (2) A fuel cell includes: (a) An anode and a cathode (b) A layer of electrolyte (c) Two resistors (d) one capacitor (3) About a bipolar plate, (a) It is used in...
10. Given that the AG for the hydrogen oxygen fuel cell reaction is -474.4 kJ/mol, calculate the E' and K for this fuel cell at 25°C: 2 H2(g) + O2(g) → 2 H20 (1)
J8-16. A hydrogen-oxygen fuel cell delivers one ampere at 0.72 V with a fuel flow of 10.00 cm3/min. Independent measurement shows that 2.25 cm/min of fuel is escaping through the electrolyte unreacted. The cell operates in the standard state of 298°K and 1 atm. (a) Find the actual voltage and current efficiency. (b) Fid the magnitude of the three major contributions to heat transfer from the cell.
3. A fuel cell designed to react grain alcohol with oxygen has the following net reaction: C2H5OH(1) + 302(g) → 2CO2(g) + 3H2O(1) The maximum work one mole of alcohol can yield by this process is 1320 kJ. What is the theoretical maximum voltage this cell can achieve?
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...
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
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...
Fuel cells can be powered by the reaction between formic acid and oxygen as following As formic acid and oxygen react together inside the fuel cell, it produced both electrical power and heat. While there is no shaft work produced by the fuel cells, this electrical power produced by the fuel cells can be considered as the shaft work term when you perform the energy balance. A fuel cell is being supplied with 100. liters per minute of pure formic...
A fuel cell designed to react grain alcohol with oxygen has the following net reaction: C2H5OH(l) + 3 O2(g) –––> 2 CO2(g) + 3 H2O(l) The maximum work that 1 mole of alcohol can yield by this process is 1320 kJ. What is the theoretical maximum voltage that this cell can achieve? NOTE: The first step in solving this problem is to determine n, the number of moles of electrons transferred when this reaction takes place as written. A) 1.14...