Question

When dinitrogen pentoxide N2O5 a white solid is heated, it decomposes to nitrogen dioxide and oxygen.
2N2O5→ 4NO2+O2
Find the volume of NO2 and O2 gases produced at S.T.P. when a sample of 54 g of N2O5 is heated.​

Answer 1

Answer:

Explanation:

Given info : When dinitrogen pentoxide (N2O5) decomposes to nitrogen dioxide and oxygen.

To find : the volume of NO₂ and O₂ gases produced when a sample 54g of N₂O₅ is heated.

Solution : 2N₂O₅ ⇒4NO₂ + O₂

Here two moles of N₂O₅ decomposes into 4 moles of NO₂ and one mole of O₂.

mass of N₂O₅ = 54g

Molecular mass of N₂O₅ = 28 + 80 = 108g

⇒no of moles of N₂O₅ = 54/108 = 0.5

so, 4 × 0.5 = 2 moles of NO₂ and 0.5 mole of O₂ are produced.

mass of NO₂ = 2 × 46 = 92 g

Mass of O₂ = 0.5 × 32= 16g

Therefore the masses of nitrogen dioxide and oxygen are 92g and 16 g respectively

Answer 2

Given: Volume of N₂O₅ = 54 grams

To find The volume of NO₂ and O₂ gases at STP.

Solution:

The following is the equation -

2N₂O₅→ 4NO₅+O₂

According to the law of conservation of mass, Two moles of N₂O₅ produce four NO₅ and one mole of O₂.

The molecular weight of  N₂O₅ = 108 grams

Number of moles of  N₂O₅ = 54/108 = 0.5

0.5 moles of N₂O₅ produce one-mole NO₅ and 0.25 moles of O₂.

One mole of any STP occupies 22.4L.

Therefore, one mole of NO₅ occupies 22.4L.

0.25 mole of Oxygen occupies 22.4×0.25L = 5.6L

Therefore, NO₂ occupies 22.4L, and Oxygen occupies 5.6L

• The mole is the base unit of the amount of substance in the International System of Units. It is defined as exactly 6.02214076×10²³ elementary entities, which may be atoms, molecules, ions, or electrons.
• The standard temperature is 273 K (0° Celsius or 32° Fahrenheit) and the standard pressure is 1 atm pressure.
• Mole is equal to the ratio of the mass of the element and molecular weight of the element.