Question

How many grams of urea ( $ N{{H}_{2}}CON{{H}_{2}} $ ) are there in 0.01 moles of it?

Answer 1

Hint: The mole is the International System of Units' basic unit of material quantity (SI). It is defined as a collection of precisely $ 6.02214076\times {{10}^{23}} $ particles, which may be atoms, molecules, ions, or electrons. For most practical applications, the value $ 6.02214076\times {{10}^{23}} $ was chosen such that the mass of one mole of a chemical compound in gram is numerically identical.

Complete Step By Step Answer:
The mole is simply a particle count. The particles being counted are usually chemically identical entities that are individually unique. A solution, for example, might include a specific number of dissolved molecules that are more or less independent of one another. The component particles of a solid, on the other hand, are stable and bonded in a lattice structure, yet they may be separated without losing their chemical identity. As a result, the solid is made up of a specific number of moles of these particles. In certain situations, such as diamond, when the entire crystal is basically a single molecule, the mole is nevertheless employed to indicate the number of atoms bonded together instead of a count of numerous molecules.
Thus, general chemical norms apply to the definition of a substance's component particles, albeit precise definitions may be required in some situations. A mole of a material has the same mass in grams as its relative atomic or molecular mass.
The molecular mass of urea is
N =2 (14) = 28
O = 1 (16) = 16
H = 4 (1) = 4
Hence its mass is 48 g/mol
We know that
 $ \text{no of moles = }\dfrac{\text{given mass}}{\text{molecular mass}} $
Where $ \text{no of moles x molecular mass = Given mass} $
So $ 0.01\times 48=0.048g $
0.048 g is the correct answer.

Note:
A substance's molar mass is the mass of one mole of that material expressed in gram multiples. The number of moles in the sample is the quantity of material. The magnitude of molar mass is numerically the same as the mean mass of one molecule, given in daltons, for most practical applications.