Question

Identify the reducing agent in the following reactions(a) 4NH3 + 5O2→ 4NO + 6H2O(b) H2O + F2 → HF + HOF(c) Fe2O3 + 3CO → 2Fe + 3CO2(d) 2H2 + O2 → 2H2ONCERT Class XScience - Exemplar ProblemsChapter_Chemical Reactions And Equations

Answer 1

Hello friend!!!

◆First find the oxidation number of each species in the reaction.

◆Secondly find the oxidation and reduction reactions.

◆The compound or element that is oxidised is the reducing agent and the one that is reduced is the oxidising agent.

●See the attachment for your answer


HOPE IT HELPS..... :-)

Answer 2

Answer:

For a: The reducing agent is Nitrogen.

For b: The reducing agent is Fluorine.

For c: The reducing agent is Carbon.

For d: The reducing agent is Hydrogen.

Explanation:

Reducing agent is defined as the agent which helps the other substance to get reduced and itself gets oxidized. The oxidation state of reducing agent gets increased.

For the given options:

• For a: $4NH_3+5O_2\rightarrow 4NO+6H_2O$

On reactant side:

Oxidation state of Nitrogen: -3

Oxidation state of Hydrogen: +1

Oxidation state of Oxygen: 0

On product side:

Oxidation state of Nitrogen: +2

Oxidation state of Hydrogen: +1

Oxidation state of Oxygen: -2

As, the oxidation state of nitrogen is increasing from -3 to +2. Thus, it is getting oxidized and is considered as an reducing agent.

• For b: $H_2O+F_2\rightarrow HF+HOF$

On reactant side:

Oxidation state of Fluorine = 0

Oxidation state of Hydrogen: +1

Oxidation state of Oxygen: -2

On product side:

Oxidation state of Fluorine: +1

Oxidation state of Hydrogen: +1

Oxidation state of Oxygen: -2

As, the oxidation state of fluorine is increasing from 0 to +1. Thus, it is getting oxidized and is considered as an reducing agent.

• For c: $Fe_2O_3+3CO\rightarrow 2Fe+3CO_2$

On reactant side:

Oxidation state of Iron = +3

Oxidation state of Carbon : +2

Oxidation state of Oxygen: -2

On product side:

Oxidation state of Iron: 0

Oxidation state of Carbon: +4

Oxidation state of Oxygen: -2

As, the oxidation state of carbon is increasing from +2 to +4. Thus, it is getting oxidized and is considered as an reducing agent.

• For d: $2H_2+O_2\rightarrow 2H_2O$

On reactant side:

Oxidation state of Hydrogen: 0

Oxidation state of Oxygen: 0

On product side:

Oxidation state of Hydrogen: +1

Oxidation state of Oxygen: -2

As, the oxidation state of Hydrogen is increasing from 0 to +1. Thus, it is getting oxidized and is considered as an reducing agent.