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

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

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?

A current of 3.6A is a passed for 6 hrs between Pt electrodes in 0.5L of 2M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

A current of 3.6A is a passed for 6 hrs between Pt electrodes in 0.5L of 2M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

A current of 3.6A is a passed for 6 hrs between Pt electrodes in 0.5L of 2M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

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)

A current of 3.7 amper is passed for 6 hre between Pt electrodes in 0.5 litre, 2M solution of Ni(NO_(3))_(2). What will be the molarity of solution at the end of electrolysis?