Question

Consider the following net ionic equation: MnO

4
−
​
(aq)+S
2−
(aq)⟶MnO
2
​
(s)+S(s) States of matter are not graded. Write the balanced equation for the reaction that takes place in acidic aqueous solution. MnO
4
−
​
(aq)+4H
+
(aq)+2 S
−2
(aq)⟶MnO
2
​
(s)+2 S(s)+2H
2
​
O(l)

Answer 1

The balanced equation for the reaction in acidic aqueous solution is MnO4- (aq) + 4H+ (aq) + 2S2- (aq) → MnO2 (s) + 2S (s) + 2H2O (l).

Step-by-step explanation:

The balanced equation for the reaction that takes place between MnO4- (aq), 4H+ (aq), and 2S2- (aq) in acidic aqueous solution is:

MnO4- (aq) + 4H+ (aq) + 2S2- (aq) → MnO2 (s) + 2S (s) + 2H2O (l)

In this balanced equation, the permanganate ion (MnO4-) is reduced to manganese(IV) oxide (MnO2), and the sulfide ion (S2-) is oxidized to sulfur (S). The presence of acid (H+) is necessary to balance the charges and ensure the reaction proceeds.

Answer 2

The balanced reaction equation is;
`2 MnO_4^- + 5 S^(2-) + 16 H^+ ---- > 2 Mn^(2+) + 8 H_2O + 5 S`

What is a balanced redox equation?

By making sure that the number of electrons gained in reduction and the number of electrons lost in oxidation are equal, a balanced redox equation accurately depicts a redox (reduction-oxidation) reaction. The oxidation half-reaction and the reduction half-reaction are the two half-reactions that make up a redox reaction.

The number of electrons gained in the reduction half-reaction and the number of electrons lost in the oxidation half-reaction are guaranteed to be equal by the balanced equation.