A solution of CuSO_(4) is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ?
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.
A 0.200M KOH solutions is electrolysed for 1.5 h using a current of 8.00 A. How many moles O_2 were produced at the anode?
Aqueous solution of CuSO_4 is electrolysed using inert electrodes till the blue coloured solution becomes colourless. The colourless solution formed is
CuSO_(4) solution is electrolysed for 15 minutes to deposity 0 . 4725 g of copper at the cathode. The current in amperes required is (Faraday = 96500 C mol^(-1) , atomic weight of copper = 63)
16 grams of copper sulphate is dissolved in one litre of water . It is electrolysed using a current strength of 10 amp for a period of 965 sec. What is the concentration of copper sulphate after electrolysis ? Take atomic weight of copper as 64 and assume there is no loss in water during electrolysis.
pH of a weakacid in 0.1 M solution is 4.3. Which statements are correct ?
100 ml, 0.1M H_2SO_4 is exactly neutralized by 100 ml of NaOH solution. Calculate the molarity of NaOH solution.
