In an electrolysis experiment, a current i passes through two different cells in series, one containing a solution of `CuSO_(4)` and the other a solution of `AgNO_(3)` . The rate of increase of the weight of the cathodes in the two cells will be

In an electrolysis experiment, current was passed for 5h through two cells connected in series. The first cell contains a solution of gold and second contains copper sulphate solution. In the first cell, 9.85g of gold was deposited. If the oxidation number of gold is +3 , find the amount of copper deposited at the cathode of the second cell. Also calculate the magnitude of the current in ampere, ( Atomic weight of Au is 1197 and atomic weight of Cu is 63.5) .

In an electrolysis experiment, current was passed for 5h through two cells connected in series. The first cell contains a solution of gold and second contains copper sulphate solution. In the first cell, 9.85g of gold was deposited. If the oxidation number of gold is +3 , find the amount of copper deposited at the cathode of the second cell. Also calculate the magnitude of the current in ampere, ( Atomic weight of Au is 1197 and atomic weight of Cu is 63.5) .

An electric current is passed through two electrolytic cells connected in series. One cell contains Cu^(2+) and the other contains Fe^(2+) . Which of the following is the correct statement?

Exactly 0.2 mole electrons are passed through two electrolytic cells in series containing CuSO_(4) and ZnSO_(4) respectively. How many grams of each metal will be deposited on the respective cathodes in the two cells ?

Exactly 0.4 faraday electric charge is passed through three electrolytic cells in series, first containing AgNO_(3) , second CuSO_(4) and third FeCl_(3) solution. How many grams of each metal will be deposited assuming only cathodic reaction in each cell ?