Question

What is the mass of the mole of sucrose $\left(C_{12}{H}_{22}{O}_{11}\right)$ ?

Answer 1

Hint: In science, the molar mass of a synthetic compound is characterized as the mass of an example of that compound partitioned by the measure of substance in that example, estimated in moles. It is the mass of one mole of the substance or $6.022\times {10}^{23}$ particles, communicated in grams.

Complete answer:
We have to know that the molar mass is a mass, not atomic, property of a substance. The molar mass is a normal of numerous examples of the compound, which frequently shift in mass because of the presence of isotopes. Most ordinarily, the molar mass is processed from the standard nuclear loads and is accordingly an earthbound normal and an element of the general wealth of the isotopes of the constituent iotas on Earth. The molar mass is proper for changing over between the mass of a substance and the measure of a substance for mass amounts.
The molecular weight is ordinarily utilized as an equivalent word of molar mass, especially for sub-atomic mixtures; in any case, the most definitive sources characterize it in an unexpected way. The equation weight is an equivalent word of molar mass that is every now, and again utilized for non-atomic mixtures, like ionic salts.
Finally the atomic mass of each atom has to be given below,
The atomic number of the atoms,
Carbon = $12$
Hydrogen = $1$
Oxygen = $16$
Then, Sucrose $\left(C_{12}{H}_{22}{O}_{11}\right)$ ,
Carbon = $12\times 12=144$
Hydrogen = $1\times 22=22$
Oxygen = $16\times 11=176$
Therefore, the total molecular mass of sucrose is $144+22+176=342g/mol$ .

Note:
We have to see that the molar mass is an escalated property of the substance, that doesn't rely upon the size of the example. In the International System of Units (SI), the lucid unit of molar mass is $kg/mol$ . Notwithstanding for chronicled reasons, molar masses are quite often communicated in $g/mol$ .