Question

What is the relative molecular weight of ${H_2}S{O_4}$ ?

Answer 1

Hint: The overall sub-atomic mass or the relative equation mass is characterized as the amount of the multitude of individual nuclear masses of all the particles in the recipe.
When sulfuric acid is a solid mineral corrosive that is dreary when unadulterated. This substance is utilized as a compound moderate to produce different synthetics and clean metal surfaces.

Complete step by step answer:
We can track down the atomic mass of the particle by following the given substance,
- Distinguish the recipe of the compound or atom.
- Utilizing the equation decides the quantity of particles present in every component of the compound or atom.
- Duplicate the nuclear load of every component with the quantity of molecules of that specific component.
- Essentially, do it for every one of the components in the atom or compound.
- Include every one of the qualities acquired in the above advance.
- At that point add the unit as grams/mole you will get the atomic mass of the substance.
The equation for sulfuric corrosive is ${H_2}S{O_4}$ .
Therefore,
The atomic mass of hydrogen is $1$ ,
The atomic mass of sulfur is $32$ ,
The atomic mass of oxygen is $16$ ,
Then we have to find the molecular weight of ${H_2}S{O_4}$ ,
$2(1){\text{ + 32 + 4(16) = 98g/mol}}$ .

Hence,
The molecular weight of ${H_2}S{O_4}$ is $98{\text{g/mol}}$ .

Note: We have to know that the sub-atomic mass and relative sub-atomic mass are particular from however identified with the molar mass. The molar mass is characterized as the mass of a given substance partitioned by the measure of a substance and is communicated in $g/mol$ . The molar mass is normally the more proper figure when managing plainly visible amounts of a substance.