Passage of charge through aqueous `CuSO_4` in the presence of Pt electrodes increases it pH value . Explain.

When propyne is treated with aqueous H_2SO_4 in the presence of HgSO_4 . the major product is

When 965 amp current is passed through aqueous solution of salt X using platinum electrodes for 10 sec, the volume of gasses liberated at the respective electrodes is in 1:1 ratio. Then X is

Predict the products of electrolysis in each of the following i) An aqueous solution of CuSO_(4) with Copper electrodes ii) An aqueous solution CuSO_(4) with plantinum electrodes

The nature of aqueous solution of CuSO_(4) , is

When the same charge is passed through the solutions of different electrolytes in series, the amounts of elements deposited in the electrodes are in the ratio of their

After the electrolysis of aqueous solution of NaCl using Pt electrodes, the pH of the solution

Same amount of electricity is passed through aqueous solutions of AgNO_3 and CuSO_4 . The number of Ag and Cu atoms deposited are x and y respectively. The correct relationship between x and y is

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte 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 proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent 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 on 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 sometimes, 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 electrolyte 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 proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent 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 on 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.