Question

Are volume fraction and mole fraction the same?

Answer 1

Hint : The mole is the International System of Units' basic unit of material quantity. It is defined as a collection of precisely $6.02214076 \times {10^{23}}$ particles, which may be atoms, molecules, ions, or electrons. The mole is a handy way to describe the quantities of reactants and products of chemical reactions in chemistry.

Complete Step By Step Answer:
The volume fraction I is defined in chemistry as the volume of a constituent Vi divided by the total volume of all constituents of the mixture V before mixing.
Its unit is 1 since it is dimensionless; it is represented as a number, such as 0.18. It's the same as volume percent (vol percent ), except that the latter has a denominator of 100, e.g., 18 percent.
In perfect solutions, when the volumes of the elements are additive, the volume fraction corresponds to the volume concentration (the volume of the solution is equal to the sum of the volumes of its ingredients).
The total of a mixture's volume fractions equals one.
$\sum\limits_{i = 1}^N {{V_i}} = V;\qquad \sum\limits_{i = 1}^N {{\phi _i}} = 1$
The mole fraction ( ${x_i}$ ) is defined as a unit of the quantity of a constituent (represented in moles), ${n_i}$ , divided by the total amount of all constituents in a mixture (also expressed in moles), ${n_{tot}}$ , in chemistry. The following is an example of this expression:
The total of all mole fractions equals 1
The mole percent, molar percentage, or molar proportion is the same idea stated with a denominator of 100. The amount fraction is another name for the mole fraction. It's the same as the number fraction, which is calculated by dividing the number of molecules of a constituent Ni by the total number of all molecules ${n_{tot}}$ .
${x_i} = \dfrac{{{n_i}}}{{{n_{{\text{tot}}}}}}$
$\sum\limits_{i = 1}^N {{n_i}} = {n_{{\text{tot}}}};\;\sum\limits_{i = 1}^N {{x_i}} = 1.$

Note :
The mole fractions and volume fractions are the same for perfect gases. When all gases are tested at the same temperature and pressure, their molar volumes are known to be the same. It's worth noting, though, that the molar masses of various gases vary.