Question

determine the oxidation states of manganese and nickel on both the reactant and predict side of the reaction. Use the activity series to determine whether the following reaction will occur or is non spontaneous. Then if it did in fact occur spontaneously what would be the oxidizing agent and reducing agent in the reaction.

Mn(s) + NiCl2 (aq) ----> MnCl2 (aq) + Ni (s)

Answer 1

Mn(s) + NiCl2 (aq) ----> MnCl2 (aq) + Ni (s)

in the reactant Mn is in 0 (zero oxidation state) and product side +2 oxidation state

in the reactant side Ni is in +2 oxidation state and in the product side Ni is in 0 (zero) oxidation state

Elements higher on the list are stronger reducing agents that elements lower down

from the activity series

Mn is above Ni in the activity series, which means it is a better reducing agent. A reducing agent gives up electrons and is therefore oxidized

reaction is spontanious

Mn is reducing agent thats why undergone oxidation

Ni+2 is oxidising agent thats why get reduced and oxidises the Mn