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The water is electrolysed in a cell, hyd...

The water is electrolysed in a cell, hydrogen is liberated at one electrode and oxygen is simultaneously liberated at the other. In a particular experiment hydrogen and oxygen so produced were collected together and the total volume measured 16.8 mL at NTP. How many coulombs were passed through the cell in the experiment ?

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To solve the problem of how many coulombs were passed through the cell during the electrolysis of water, we can follow these steps: ### Step-by-Step Solution: 1. **Understand the Reaction**: - During the electrolysis of water, hydrogen (H₂) is produced at the cathode and oxygen (O₂) at the anode. The balanced chemical equation for the electrolysis of water is: \[ 2H_2O(l) \rightarrow 2H_2(g) + O_2(g) ...
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A certain amount of charge is passed through acidulated water. A total of 504mL of hydrogen and oxygen were collected at STP. Find the magnitude of charge that is passed during electrolysis in coulombs.

During the electrolysis of water, a total volume of 33.6mL of hydrogen and oxygen gas was collected at STP . Find the amound of electricity that passed during electrolysis.

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. The platinum electrodes were immersed in a solution of cupric sulphate (CuSO_(4)) and electric current is passed through the solution. after sometime, it was observed that the colour of copper sulphate disappeared with evolution of a gas at the electrode. The colourless solution contains :

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. The quantity of electricity required to liberate 112 cc hydrogen at S.T.P. from acidified water is :

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. Calculate the volume of gas liberated at the anode at STP during the electrolysis of a CuSO_(4) solution by a current of 1 A passed for 16 minutes and 5 seconds :

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A silver coulometer is in series with a cell electrolyzing water. In a time of 1 minute at a constant current 1.08 g silver get deposited on the cathode of the coulometer. What total volume (in mL at 1atm, 273K) of the gases would have produced in other cell. In this cell that the anodic and cathodic efficiencies were 90% and 80% respectively. Assume the gases collected are dry. (Ag = 108) (molar volume of any ideal gas at 1atm and 273K = 22.4L)

RC MUKHERJEE-ELECTROLYSIS AND ELECTROLYTIC CONDUCTANCE-Problems
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  2. How many grams of H(2) and O(2) are produced during the electrolysis o...

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  3. The water is electrolysed in a cell, hydrogen is liberated at one elec...

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  6. A current of 0.5 amp is sent through a solution of CuSO(4) for 20 minu...

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  8. How many hour are required for a current of 3.0 ampere to decompose 18...

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  9. 50 mL of a 0.1 M CuSO(4) solution is electrolysed for 12 minutes at a ...

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