A current of 2.0A is used to plate Ni(s) from 500mL of a 1.0M `Ni^(2+)`(aq) solution. What is the `[Ni^(2+)]` after 3.0 hours?

A current of 12A is used to plate nickel from a Ni(NO_(3))_(2) solution. Both Ni(s) and H_(2)(g) are produced at the cathode. If the current efficiency with respect to the formation of Ni(s) is 62%, how many grams of nickel are plated on the cathode in 45minutes?

A current of 3.7 A is passed for 6hrs. Between Ni electrodes in 0.5 L of 2 M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

It takes 126.5 minutes using a current of 5.15 A to deposit all of the nickel from 225mL of a solution contaiing Ni^(2+) . What was the original concentration of Ni^(2+) in the solution?

A current of 3.7 A is passed for six hours between Ni electrodes in 0.5 L of 2M solution of Ni(NO_(3))_(2) . The molarity of solution at the end of electrolysis will ___________.

A current of 3.7 ampere is passed for 6 hours between platinum electrodes in 0.5 litre of a 2 M solution of Ni(NO_(3))_(2) . What will be the molarity of the solution at the end of electrolysis ? What will be the molarity of the solution if nickel electrodes are used ? (1 F=96500 coulomb, Ni=58.7)