Volume Fraction To Mass Fraction Top 8 Latest Posts

The conversion from volume fraction to mass fraction depends on the density of the material in question.

To convert from volume fraction to mass fraction, you can use the following formula:

Mass fraction = (Volume fraction x Density) / 100

Where:

• Volume fraction is the proportion of the volume of the material in question that is occupied by the substance of interest
• Density is the mass per unit volume of the material in question, usually measured in kg/m³ or g/cm³.

For example, let’s say you have a solution with a volume fraction of 20% of ethanol in water. The density of ethanol is 0.789 g/cm³ and the density of water is 1 g/cm³. To convert the volume fraction of ethanol to its mass fraction, you would use the following calculation:

Mass fraction of ethanol = (Volume fraction of ethanol x Density of ethanol) / (Volume fraction of ethanol x Density of ethanol + Volume fraction of water x Density of water)
= (0.2 x 0.789) / (0.2 x 0.789 + 0.8 x 1)
= 0.135

Therefore, the mass fraction of ethanol in this solution is 13.5%.

To convert volume fraction to mass fraction, you need to know the density of the substance in question. The formula for the conversion is:

Mass Fraction = (Volume Fraction x Density) / 100

where:

• Volume Fraction is the percentage of the volume that a substance occupies in a mixture
• Density is the mass per unit volume of the substance

To use the formula, simply plug in the values and solve for the mass fraction.

For example, let’s say we have a mixture of ethanol and water with a volume fraction of ethanol of 20%. The density of ethanol is 0.789 g/mL and the density of water is 1 g/mL. To convert the volume fraction of ethanol to its mass fraction, we would use the formula as follows:

Mass Fraction = (20 x 0.789) / (20 x 0.789 + 80 x 1) x 100
Mass Fraction = 13.26%

Therefore, the mass fraction of ethanol in the mixture is 13.26%.

To convert volume fraction to mole fraction, we need to know the densities and molecular weights of the substances involved.

Assuming we have a mixture of two substances A and B, with volume fractions VA and VB respectively, and densities ρA and ρB, and molecular weights MA and MB respectively, we can use the following equation to convert volume fraction to mole fraction:

mole fraction of A = VA × ρB × NA / (VB × ρA × MA + VA × ρB × NA)
where NA is Avogadro’s number (6.022 x 10^23).

Similarly, mole fraction of B = 1 – mole fraction of A

For example, if we have a mixture of ethanol (C2H5OH) and water (H2O) with volume fractions of ethanol and water as 0.4 and 0.6 respectively, and the densities of ethanol and water are 0.789 g/cm^3 and 1 g/cm^3 respectively, and their molecular weights are 46.07 g/mol and 18.02 g/mol respectively, then the mole fraction of ethanol can be calculated as follows:

mole fraction of ethanol = 0.4 × 1 g/cm^3 × 6.022 × 10^23 / (0.6 × 0.789 g/cm^3 × 46.07 g/mol + 0.4 × 1 g/cm^3 × 6.022 × 10^23)
= 0.501

Therefore, the mole fraction of ethanol in the mixture is 0.501 and the mole fraction of water would be 1 – 0.501 = 0.499.