Question

What amount of atoms, in mol, is present in 128g of sulphur dioxide? Why?

Answer 1

In order to answer the query, we must first describe what sulphur dioxide is and how to measure it, as well as provide a proper description and characteristics. As an example, we can claim that the chemical formula we would use to calculate mass =$mole \times molecular{\text{ atoms}} \times {\text{6}}{\text{.022}} \times {\text{1}}{{\text{0}}^{23}}$ .

Complete answer:
The given question statement asks about the sulphur dioxide and the main concepts of the moles and subsequently the molecular atoms of sulphur dioxide. Which should be determined in a step by step process.
Sulphur dioxide is the chemical compound with the chemical formula of $S{O_2}$ and in uses it is a toxic gas responsible for the smell of burnt matches. It is released naturally by volcanic activity and is produced as a by-product of copper extraction and the burning of fossil fuels contaminated with sulfur compounds. Sulfur dioxide has a pungent smell like nitric acid.
Now we have to give the step by step solution of the problem.
Step 1:
We have to find the 1 mole molecular mass of the $S{O_2}$ which should be the addition of the atoms of the sulphur dioxide.
This would be $= 32 \times 1 + 16 \times 2 = 64g$
Step 2:
Now the mass of the 1 mole $S{O_2}$ is $= 64g$
So the number of moles would be the division of the molecular mass and the total given mass.
$= \dfrac{{128}}{{64}} \\\ = 2moles \\\$
Step 3:
Now we have to use the given formula of $mole \times molecular{\text{ atoms}} \times {\text{6}}{\text{.022}} \times {\text{1}}{{\text{0}}^{23}}$ to find the answer:
$= mole \times molecular{\text{ atoms}} \times {\text{6}}{\text{.022}} \times {\text{1}}{{\text{0}}^{23}} \\\ = 2 \times 3 \times {\text{6}}{\text{.022}} \times {\text{1}}{{\text{0}}^{23}} \\\ = 3.613 \times {\text{1}}{{\text{0}}^{24}} \\\$
Therefore the answer for the given problem is $= 3.613 \times {\text{1}}{{\text{0}}^{24}}atoms$ .

Note:
On other planets, sulfur dioxide can be found in various concentrations, the most significant being the atmosphere of Venus, where it is the third-most significant atmospheric gas at 150 ppm. There, it condenses to form clouds, and is a key component of chemical reactions in the planet's atmosphere and contributes to global warming.