Determine the combined pressure exerted by a blend of 0.45 kg mole of benzene, 0.44 kg mole of toluene, and 0.23 kg mole of o-xylene at 100°C, given their individual vapor pressures at 100°C are 1340, 560, and 210 mmHg respectively.
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Answer: C. 801.5
Explanation
Dalton law states that total vapor pressure equals the sum of partial pressures exerted by each individual component. Partial pressure for each aromatic hydrocarbon is calculated by multiplying its mole fraction by its pure vapor pressure. Summing the partial pressure contributions of benzene, toluene, and o xylene yields approximately eight hundred one point five millimeters. Mole fractions are determined by dividing individual component moles by the total number of moles in the liquid mixture. Total moles equal the sum of zero point four five, zero point four four, and zero point twenty three moles. Vapor pressure data at specific temperatures allows engineers to model ideal liquid vapor phase equilibrium systems accurately.
Option A undercalculates the total pressure by omitting correct fractional contributions from the heavier hydrocarbon components. Option B fails to match the precise summation of partial pressures derived from correct mole fraction calculations. Option D overestimates the combined pressure by miscalculating individual partial pressure contributions in the mixture.
- Subject
- Engineering
- Category
- Chemical Engineering
- Topic
- —
- Difficulty
- medium
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