Question

Consider the following reaction and select the false statement below.

10 I−(aq) + 16 H+(aq) + 2 MnO4−(aq) → 5 I2(s) + 2 Mn2+(aq) + 8 H2O(l)

(A) this is a reduction-oxidation (redox) reaction
(B) the iodine ion is the reducing agent
(C) the permanganate ion is the oxidizing agent
(D) the hydrogen ion is neither reduced nor oxidized
(E) in the reaction as written, ten moles of electrons are transferred from the oxidizing agent to the reducing agent

Answer 1

Answer: The correct answer is Option E.

Step-by-step explanation:

Redox reaction is defined as the reaction in which oxidation and reduction reaction occur simultaneously.

Oxidation reaction is defined as the reaction in which a chemical species looses its electrons. Here, oxidation state of the species increases.

`X\rightarrow X^(n+)+ne^-`

Reduction reaction is defined as the reaction in which a chemical species gains electrons. Here, the oxidation state of the species decreases.

`X^(n+)+ne^-\rightarrow X`

Oxidizing agents are the agents that oxidizes the other substance and itself gets reduced. These agents undergoes reduction reactions.

Reducing agents are the agents that reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

For the given chemical reaction:

`10I^-(aq.)+16H^+(aq.)+2MnO_4^-(aq.)\rightarrow 5I_2(s)+2Mn^(2+)(aq.)+8H_2O(l)`

The half reaction follows:

Oxidation half reaction:
`2I^-\rightarrow I_2+2e^-` ( × 5)

Reduction half reaction:
`MnO_4^-(aq.)+8H^+(aq.)+5e^-\rightarrow Mn^(2+)(aq.)+4H_2O` ( × 2)

As, iodine ion is getting oxidized. So, it is considered as a reducing agent and permanganate ion is considered as an oxidizing agent.

Electrons in a redox reaction is transferred from the substance getting oxidized (reducing agent) to the substance getting reduced (oxidizing agent)

Hence, the correct answer is Option E.