Among the following cells
Leclanche cell (I)
Nickel–cadmium cell (II)
Lead storage battery (III)
Mercury cell (IV)
Primary cells are
Among the following cells
Leclanche cell (I)
Nickel–cadmium cell (II)
Lead storage battery (III)
Mercury cell (IV)
Primary cells are
The hydrogen electrode is dipped in a solution of pH 3 at 25°C. The potential would be (the value of 2.303 RT/F is 0.059 V) |
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When same quantity of electricity is passed for half an hour, the amount of Cu and Cr deposited are respectively 0.375 g and 0.30 g. Ratio of electrochemical equivalent of Cu and Cr is |
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Given the data at 25°C, Ag + I– → AgI + e– ; E° = 0.152 V Ag → Ag+ + e–; E° = –0.800 V What is the value of log Ksp for AgI? $\left(2.303dfrac{ ext{RT}}{ ext{F}} = 0.059 ext{ V} ight)$ |
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The quantity of electricity needed to separately electrolyze 1 M solution of ZnSO4, AlCl3 and AgNO3 completely is in the ratio of |
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An infinite dilution of aqueous solution of BaCl2, molar conductivity of Ba2+ and Cl– ions are = 127.32 S cm2/moland 76.34 S cm2/mol respectively. What is Λ∞ |
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Aqueous copper sulphate solution is electrolyzed using platinum electrodes. The electrode reaction occurring at cathode is |
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Zn | Zn2+ (a = 0.1M) || Fe2+ (a = 0.01M) | Fe. The emf of the above cell is 0.2905 V. Equilibrium constant for the cell reaction is |
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Calculate the reduction potential of a half–cell containing platinum electrode immersed in 2.0 M Fe2+ and 0.02 M Fe3+. Given Eo Fe3+ + e– → Fe2+ |
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Consider the following four electrodes, P = Cu2+ (0.0001 M) | Cu(s) Q = Cu2+ (0.1 M) | Cu(s) R = Cu2+ (0.01 M) | Cu(s) S = Cu2+ (0.001 M) | Cu(s) If the standard reduction potential of Cu2+/Cu is +0.34 V, the reduction potentials in volts of the above electrodes follow the order |
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Conductivity of 0.01 M NaCl solution is 0.00147 ohm–1cm–1. What happens to this conductivity if extra 100 ml of H2O will be added to the above solution? |
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