Hydrogen gas is not liberated when the following metal is added to dil. HCl.
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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Which of the following electrolytic solutions has the least specific conductance? |
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The standard electrode potential for the half cell reactions are Zn++ + 2e– → Zn, E° = – 0.76 V Fe++ + 2e– → Fe, E° = – 0.44 V The e.m.f. of the cell reaction Fe++ + Zn → Zn++ + Fe is |
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