Assertion (A) : A current of 96.5 A is passed into aqueous AgNO_(3) solution for 100s. The weight of silver deposited is 10.8g (at. wt. of Ag =108). Reason (R) : The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte. The correct answer 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. 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.
The weight in grams of O_2 formed at Pt anode during the electrolys of aq. K_2 SO_4 solution during the passage of one coulomb of electricity is
What are the products obtained at the cathode and anode during the electrolysis of the following when platinum electrodes are used in the electrolysis a) Molten b) Aq. CuSO_(4) solution c) Aq. K_(2)SO_(4) solution
write the question for reaction of zinc with hydrochloric acid and balance the equation find out the number of molecules of hydrogen gas produced in this reaction, when 5 mole of HCL completely reacts at STP (Gram molar volume is 22.4 litres at STP, Avogadro’snumber is 6.023 xx 10^(23)
1.15 g of an organic compound was analysed by Kjeldahl's method and the ammonia produced was collected in 30 mL of normal HCl solution. The excess of acid consumed 18.4 mL of normal sodium hydroxide solution for back titration. Calculate the percentage of nitrogen in the substance.
An acidic solution of Cu^(2+) salt containing 0.4 g of Cu^(2+) is electrolysed until all the copper is deposited. The electrolysis is continued for seven more minutes with the volume of solution kept at 100 ml and the current at 1.2 amp. Calculate the volume of gases evolved at NTP during the entire electrolysis.
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 passage of current liberates H_2 at cathode and Cl_2 at anode. The solution is
