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Chromium metal can be plated out from an acidic solution containing ${CrO}_{3}$ according to the following equation.

${CrO}_{3} (aq) + 6 H_{}^{+} (aq) + 6 e^{-} \to Cr (s) + 3 H_{2} O$

Determine the following :

(i) The amount of chromium that will be plated out by $24, 000$ coulombs.

(ii) The time it will take to plate out $1.5 g$ of chromium by using $12.5 amp$ current.

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Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing

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The density of metal and equivalent weight of a metal are

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How long (approximate) should water be electrolysed by passing through

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The weight of silver (at.wt.

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When

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

A current of $10.0 A$ flows for $2.00 h$ through an electrolytic cell containing a molten salt of metal $X$ . This results in the decomposition of $0.250 mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is:

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

The quantity of electricity needed to separately electrolyse

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{AgNO}_{3}

completely is in the ratio of

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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250 s

through

250 m L of 0.15 M

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M S O_{4} .

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of the current was utilised for electrolysis. The molarity of

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An aqueous solution of

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A constant current (0.5 amp) is passed for 1 hour through (i) aqueous

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

One litre solution of

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

A solution of

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

The number of Faradays(F) required to produce

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

Calculate the molarity of a solution containing

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dissolved in the product of a

H_{2} - O_{2}

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1 A

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595.1

hours.

(Assume

1 F = 96500 C / m o l

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40 g m o l^{- 1}

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

During the electrolysis of molten sodium chloride, the time required to produce

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Important Questions on Electrochemistry

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