(a) What volume of H2(g), stored at 31°C at a pressure of 149 atm, would be needed to run an electric motor drawing a current of 9.2 A for 1.5 h? ____ L(b) What volume (liters) of air at 27°C and 1.47 atm will have to pass into the cell per minute to run the motor? Assume that air is 20. percent O2 by volume and that all the O2 is consumed in the cell. The other components of air do not affect the fuel-cell reactions. Assume ideal gas behavior. ___ L/min
For (a), 1. calculate the number of coulombs of electricity that pass through the cell ?C 9.2A * 1.5h *3600s 49680C 2. convert to number of moles of electrons 49680C * (1 mole e/ 96500 C) 0.5148 3. Ans * (1 mol H2/ 2 mol e) 0.2574 mol this is the n we need 4. use the equation V nRT/P For (b) I'm still working on it Good luck!
