Advertisements
Advertisements
प्रश्न
In \[\ce{H2 - O2}\] fuel cell the reaction occurs at cathode is:
पर्याय
\[\ce{O2_{(g)} + 2H2O_{(l)} + 4e^- -> 4OH^-_{( aq)}}\]
\[\ce{H^+_{( aq)} + OH^-_{( aq)} -> H2O_{(l)}}\]
\[\ce{2H2_{(g)} + O2_{(g)} -> 2H2O_{(g)}}\]
\[\ce{H^+ + e^- -> 1/2H2}\]
Advertisements
उत्तर
\[\ce{O2_{(g)} + 2H2O_{(l)} + 4e^- -> 4OH^-_{( aq)}}\]
APPEARS IN
संबंधित प्रश्न
The button cell used in watches functions as follows.
\[\ce{Zn_{(s)} + Ag2O_{(s)} + H2O_{(l)} ⇌ 2Ag_{(s)} + Zn^{2+}_{( aq)} + 2OH^-_{( aq)}}\] the half cell potentials are \[\ce{Ag2O_{(s)} + H2O_{(l)} + 2e^- -> 2Ag_{(s)} + 2OH^-_{( aq)}}\] E0 = 0.34 V The cell potential will be
During electrolysis of molten sodium chloride, the time required to produce 0.1 mole of chlorine gas using a current of 3A is ___________.
The number of electrons delivered at the cathode during electrolysis by a current of 1A in 60 seconds is ____________.
(charge of electron = 1.6 × 10−19 C)
While charging lead storage battery
Among the following cells
I) Leclanche cell
II) Nickel – Cadmium cell
III) Lead storage battery
IV) Mercury cell
Primary cells are:
For the cell reaction
\[\ce{2Fe^{3+}_{( aq)} + 2l^-_{( aq)} -> 2Fe^{2+}_{( aq)} + l2_{( aq)}}\]
\[\ce{E^0_{cell}}\] = at 298 K. The standard Gibbs energy (∆G°) of the cell reactions is:
State Faraday’s Laws of electrolysis.
A current of 1.608A is passed through 250 mL of 0.5 M solution of copper sulphate for 50 minutes. Calculate the strength of Cu2+ after electrolysis assuming volume to be constant and the current efficiency is 100%.
The same amount of electricity was passed through two separate electrolytic cells containing solutions of nickel nitrate and chromium nitrate respectively. If 2.935 g of Ni was deposited in the first cell. The amount of Cr deposited in the another cell?
Given: molar mass of Nickel and chromium are 58.74 and 52 gm−1 respectively.
Explain the function of H2 – O2 fuel cell.
