An Ideal solution is formed by mixing 0.26 mol of pentane (vapor pressure + 511 torr) with 0.34 mol of hexane (vapor pressure = 150 torr). What is the total vapor pressure of the ideal solution?
If those are partial pressures of each material then the Ptotal = ppentane + phexane
To find the total vapor pressure of the ideal solution, we can use Raoult's law. According to Raoult's law, the vapor pressure of a component in an ideal solution is proportional to its mole fraction in the mixture.
The mole fraction (X) of a component can be calculated by dividing the moles of that component by the total moles of all components in the solution.
Step 1: Calculate the mole fraction of pentane:
Mole fraction (X) of pentane = moles of pentane / total moles
= 0.26 mol / (0.26 mol + 0.34 mol)
= 0.26 mol / 0.60 mol
= 0.4333
Step 2: Calculate the mole fraction of hexane:
Mole fraction (X) of hexane = moles of hexane / total moles
= 0.34 mol / (0.26 mol + 0.34 mol)
= 0.34 mol / 0.60 mol
= 0.5667
Step 3: Use the mole fractions to calculate the partial pressures of each component:
Partial pressure of pentane = mole fraction of pentane * vapor pressure of pentane
= 0.4333 * 511 torr
= 221.2 torr
Partial pressure of hexane = mole fraction of hexane * vapor pressure of hexane
= 0.5667 * 150 torr
= 85.0 torr
Step 4: Add the partial pressures to find the total vapor pressure of the ideal solution:
Total vapor pressure = partial pressure of pentane + partial pressure of hexane
= 221.2 torr + 85.0 torr
= 306.2 torr
Therefore, the total vapor pressure of the ideal solution is 306.2 torr.