Question

Consider the following general voltaic cell and a cell notation, and answer all three parts of this question.

Answer 1

Answer:

Part -1

Electrode A - Mg(s)

Electrode B - $Cl_{2}$

Part-2

Option -C

Part - 3

Electrons flow from electrode -A to electrode -B.

Explanation:

Part-1

Electrode A is $Mg(s)|Mg^{+2}(aq)$

Electrode B is $Cl_{2}(g)|Cl^{-}(aq)|C(s)$

Part-2

From the electrode, magnesium looses two electrons and chlorine gains two electrons. Therefore, balanced redox equation for the voltaic cell is as follows.

$Mg(s)+Cl_{2}(g)\rightarrow Mg^{2+}(aq)+2Cl^{-}(aq)$

Part-3

$Na^{+}$ ions flow from the left to right.

$NO_{3}^{-}$ ions flow from the right to left.

Therefore, Electrons flow from electrode -A to electrode -B.