Electrolysis of a molten salt with the formula mcl, using a current of 3.86 amp for 16.2 min, deposits 1.52 g of metal. identify the metal. (1 faraday = 96,485 coulombs) a) li b) na c) k d) rb e) ca

Option (c) is the correct answer.

Explanation:

It is known that relation between charge, current and time is as follows.

   Total charge passed = current (A) x time (s)

                      =

                    = 3751.92 C

Moles of electrons passed =

                                             =

                                            = 0.03889 mol

As, the given metal salt is MCl. Therefore, the reduction reaction is as follows.

Thus, moles of M = moles of electrons = 0.03889 mol

As we known that molar mass is calculated using the formula:

     Molar mass of M =

                                  =

                                 = 39.1 g/mol

We know that potassium is the metal which has molar mass as 39 g/mol.

Thus, we can conclude that the metal is identified as K (potassium).

the answer is b. dilution