Advertisements
Advertisements
प्रश्न
Calculate the standard emf of the cell: \[\ce{Cd|Cd^{2+}||Cu^{2+}|Cu}\] and determine the cell reaction. The standard reduction potentials of Cu2+|Cu and Cd2+|Cd are 0.34 V and −0.40 volts respectively. Predict the feasibility of the cell reaction.
Advertisements
उत्तर
Cell reactions:
Oxidation at anode:
\[\ce{Cd_{(s)} -> Cd^{2+}_{( aq)} + 2e^-}\] \[\ce{(E^0_{ox})_{{Cd|Cd^{2+}}}}\] = 0.4 V
Reduction at cathode:
\[\ce{Cu^{2+}_{( aq)} + 2e^- -> Cu_{(s)}}\] \[\ce{(E^0_{red})_{{Cu^{2+}|Cu}}}\] = 0.34 V
\[\ce{Cd_{(s)} + 2e^- -> Cd^{2+}_{( aq)} + Cu_{(s)}}\]
`"E"_"cell"^0 = ("E"_"ox"^0)_"anode" + ("E"_"red"^0)_"cathode"`
= 0.4 + 0.34
= 0.74 V
emf is +ve, so ΔG is (−)ve, the reaction is feasible.
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
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:
In \[\ce{H2 - O2}\] fuel cell the reaction occurs at cathode is:
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.
In fuel cell H2 and O2 react to produce electricity. In the process, H2 gas is oxidised at the anode and O2 at cathode. If 44.8 litre of H2 at 25°C and 1 atm pressure reacts in 10 minutes, what is average current produced? If the entire current is used for electro deposition of Cu from Cu2+, how many grams of deposited?
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.
8.2 × 1012 litres of water is available in a lake. A power reactor using the electrolysis of water in the lake produces electricity at the rate of 2 × 106 Cs−1 at an appropriate voltage. How many years would it like to completely electrolyse the water in the lake? Assume that there is no loss of water except due to electrolysis.
Explain the function of H2 – O2 fuel cell.
