Given the reaction below: N2 (9)
+
(g) + N205 (9)
What is the oxidizing agent of the reaction?

The oxidizing agent of the reaction : O₂

Given

Reaction

N₂ + O₂ ⇒ N₂O₅

Required

The oxidizing agent

Solution

The balanced equation :

2N₂ + 5O₂ ⇒ 2N₂O₅

Oxidation is an increase in oxidation number, while reduction is a decrease in oxidation number.

In the redoxs reaction, it is also known  :

The reducing agents : a substance that experience oxidation

The oxidizing agent : a substance that is reduced

2N₂  → 2N₂O₅ (oxidation of N)

0 to +5

5O₂  → 2N₂O₅ (reduction of O)

0 to -2

So N₂ reducing agent, O₂ an oxidizing agent.

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm