The half cell reaction, with its standard reduction potentials are:
(i) Pb2++ 2e– → Pb (E° = –0.13 V)
(ii) Ag++ e– → Ag (E° = +0.80 V)
Which ofthe following reactions will occur?
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Given Eo The value of standard electrode potential for the change, Fe3+(aq) + e– → Fe2+ will be |
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Hydrogen gas is not liberated when the following metal is added to dil. HCl. |
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Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is (1 Faraday = 96500 C mol–1) |
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Given Eo the potential for the cell Cr / Cr3+ (0.1 M) || Fe2+ (0.01 M) | Fe is |
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Calculate Λ∞ HoAc using appropriate molar conductances of the electrolytes listed above at infinite dilution in H2O at 25°C |
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The equivalent conductances of two strong electrolytes at infinite dilution in H2O (where ions move freely through a solution) at 25°C are given below: Λo Λo What additional information/quantity one needs to calculate Λ° of an aqueous solution of acetic acid? |
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In a cell that utilizes the reaction Zn(s) + 2H+ (aq) → Zn2+ (aq) + H2(g) addition of H2SO4 to cathode compartment will |
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For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46 V at 25°C. The value of standard Gibbs energy, ΔG° will be (F = 96500 C mol–1) |
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In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under S.T.P. conditions. The current to be passed is |
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The one which decreases with dilution is |
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