An aqueous sol of `CuSo_4` measuring 1 L was electrolysed till the ph of solution was found to be 1 then amount of Cu deposited and volume of gas evolved (at STP) are respectively(Cu=63.5g/mol)

A solution of CuSO_(4) is electrolyzed for 10 min with a current of 1.5A . What is the mass of Cu deposited at the cathode? [ Atomic mass of Cu=63g]

An acidic solution of Cu^(2+) ions containing 0.4 g of Cu^(2+) ions is electrolysed until all the copper is deposited. Calculate the volume of oxygen evolved at N.T.P.

During electrolysis of an aqueous solution of CuSO_(4) using copper electrodes, if 2.5g of Cu is deposited at cathode, then at anode

A solution of CuSO_(4) is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)

A solution of CuSO_(4) is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)

An acidic solution of Cu^(2+0 salt containing 0.4g of Cu^(2+) is electrolyzed until all the copper is deposited. The electrolysis is continued for seven more minutes with the volume of solution kept at 100mL and the current at 1.2A . Calculate the volume of gases evolved at STP during the entire electrolysis.

In the electrolysis of 7.2L aqueous solution of CuSO_(4) , a current of 9.65A passed for 2 hours. Find the weight of Cu deposited at cathode.

Two faraday of electricity is passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode is: (at mass of Cu = 63.5 amu)

1.0 L of 0.1 M aqueous solution of KCI is electrolysed A current of 96.50 mA is passed through the solutoin for 10 hour which is /are correct ? (assume volume of soluto remains constant during electrolysis)

The strength in volumes of a solution containing 30.36 g/L of H_(2)O_(2) is (Given volume of 1 mole of gas STP = 22.4 litre)