Explain how rusting of iron is envisaged as setting up of an electrochemical cell.
In the electrochemical cell H_(2)(g) 1atm | 1H^(+)(lm) || Cu^(2+) (IM) |Cu(s) Which one of the following statements is true?
hydrogen-oxygen fuel cell may have an acidic or alkaline electrolyte. The half-cell reactions are To maximize the power per unit mass of an electrochemical cell, the electronic and electrolytic resistances of the cell must be minimized. Since fused salts have lower electrolytic resistances that aqueous solutions, high-temperature electrochemical cells are of special interest for practical applications. High temperature also allow the use of liquid metal electrode, which make possible higher current densities than solid electrodes How many grams of water is produced in the cell if 2 Faradays of charge is derived from the fuel cells
hydrogen-oxygen fuel cell may have an acidic or alkaline electrolyte. The half-cell reactions are To maximize the power per unit mass of an electrochemical cell, the electronic and electrolytic resistances of the cell must be minimized. Since fused salts have lower electrolytic resistances that aqueous solutions, high-temperature electrochemical cells are of special interest for practical applications. High temperature also allow the use of liquid metal electrode, which make possible higher current densities than solid electrodes If 560 mL of H_2 gas at STP is fed into and is consumed by the fuel cell in 10 minutes, then what is the current output of the fuel cell?
hydrogen-oxygen fuel cell may have an acidic or alkaline electrolyte. The half-cell reactions are To maximize the power per unit mass of an electrochemical cell, the electronic and electrolytic resistances of the cell must be minimized. Since fused salts have lower electrolytic resistances that aqueous solutions, high-temperature electrochemical cells are of special interest for practical applications. High temperature also allow the use of liquid metal electrode, which make possible higher current densities than solid electrodes For a Hydrogen-Oxygen fuel cell if DeltaH_(f)^(@)=(H_2O, l) = – 285 kJ //" mole" , then what will be its thermodynamic efficiency under standard conditions
Explain with a suitable example the relation between the gibbs energy of chemical reaction (G) and the functioning of the electrochemical cell.
For the electrochemical cell M// M^(+) // // X^(-) // X , E^(0) M^(+)// M = 0.44 V and E^(0) (x//x^(-)) = 0.33 V . From the one can deduce that
The electrochemical cell shown below is a concentration cell. M|M^(2+) (saturated solution of a sparingly soluble salt, MX_2 || M^(2+) (0.001 mol dm^(-3) ) |M The emf of the cell depends on the difference in concentration of M^(2+) ions at the two electrode The emf of the cell at 298 is 0.059 V The value of DeltaG (kJ " mol"^(-1)) for the given cell is ( take 1F = 96500 C " mol"^(-1) )
