No, you cannot directly determine partial pressures from volume fractions alone. Partial pressures are related to the mole fractions or concentrations of the individual components in a gas mixture, not the volume fractions.
Mole fractions and volume fractions are not the same, although they are related.
Mole fraction (also known as the mole fraction or the amount fraction) is a measure of the relative number of moles of a component in a mixture. It is calculated by dividing the number of moles of a specific component by the total number of moles in the mixture.
Volume fraction (also known as the volume percent or volume ratio) is a measure of the relative volume of a component in a mixture. It is calculated by dividing the volume of a specific component by the total volume of the mixture and multiplying by 100 to express it as a percentage.
While volume fraction provides information about the relative volumes of components in a mixture, it does not directly give information about the number of moles or the concentration of the components. To determine partial pressures, mole fractions are typically used.
To convert from volume fraction to mole fraction, you need to know the molar volume (volume occupied by one mole) of the components. Once you have the mole fractions, you can use them to calculate partial pressures using Dalton's law of partial pressures, which states that the total pressure of a mixture of non-reacting gases is the sum of the partial pressures of the individual gases.
In summary, while volume fractions and mole fractions are related, they are not the same. Volume fractions provide information about the relative volumes of components, whereas mole fractions are used to determine the relative number of moles or concentrations of components in a mixture. Partial pressures are determined using mole fractions rather than volume fractions.