Vapour pressure of benzene and toluene are 0.9bar and 0.85bar. 7.8g of benzene is added to 180g of toluene. To find the vapour pressure of the resultant solution
To find the vapor pressure of the resultant solution, we can use Raoult's law, which states that the vapor pressure of a solution is equal to the mole fraction of each component multiplied by its pure component vapor pressure.
First, let's find the mole fraction of benzene and toluene in the solution.
The number of moles of benzene can be calculated using its molar mass:
moles of benzene = mass of benzene / molar mass of benzene
moles of benzene = 7.8g / 78.11 g/mol (molar mass of benzene)
moles of benzene = 0.1 mol
The number of moles of toluene can be calculated using its molar mass:
moles of toluene = mass of toluene / molar mass of toluene
moles of toluene = 180g / 92.14 g/mol (molar mass of toluene)
moles of toluene = 1.95 mol
Now, we can calculate the mole fraction of each component:
mole fraction of benzene = moles of benzene / total moles
mole fraction of benzene = 0.1 mol / (0.1 mol + 1.95 mol)
mole fraction of benzene = 0.049
mole fraction of toluene = moles of toluene / total moles
mole fraction of toluene = 1.95 mol / (0.1 mol + 1.95 mol)
mole fraction of toluene = 0.951
Finally, we can calculate the vapor pressure of the resultant solution using Raoult's law:
vapor pressure of resultant solution = (mole fraction of benzene) * (vapor pressure of benzene) + (mole fraction of toluene) * (vapor pressure of toluene)
vapor pressure of resultant solution = (0.049) * (0.9 bar) + (0.951) * (0.85 bar)
vapor pressure of resultant solution = 0.0441 bar + 0.80935 bar
vapor pressure of resultant solution = 0.85345 bar
Therefore, the vapor pressure of the resultant solution is approximately 0.85345 bar.
To find the vapor pressure of the resultant solution, we need to consider the concept of Raoult's Law, which states that the partial pressure of each component in an ideal solution is directly proportional to its mole fraction.
First, we need to calculate the mole fraction of benzene and toluene in the solution.
Mole fraction of benzene (Xbenzene) = number of moles of benzene / total number of moles
To calculate the number of moles of benzene, we'll use the formula:
number of moles = mass of substance / molar mass
The molar mass of benzene (C6H6) is 78 g/mol.
Number of moles of benzene = 7.8g / 78g/mol = 0.1 mol
Now, let's calculate the number of moles of toluene:
The molar mass of toluene (C7H8) is 92 g/mol.
Number of moles of toluene = 180g / 92g/mol = 1.96 mol
Next, we can calculate the mole fraction of toluene:
Xtoluene = number of moles of toluene / total number of moles
Total moles = moles of benzene + moles of toluene = 0.1 mol + 1.96 mol = 2.06 mol
Xtoluene = 1.96 mol / 2.06 mol = 0.951
Now, we can use Raoult's Law to find the vapor pressure of the resultant solution:
Vapor pressure of resultant solution = Xbenzene * vapor pressure of benzene + Xtoluene * vapor pressure of toluene
Using the given values:
Vapor pressure of benzene = 0.9 bar
Vapor pressure of toluene = 0.85 bar
Vapor pressure of resultant solution = (0.1 * 0.9) + (0.951 * 0.85)
Vapor pressure of resultant solution = 0.09 + 0.80835
Vapor pressure of resultant solution = 0.89835 bar
Therefore, the vapor pressure of the resultant solution is approximately 0.89835 bar.
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The partial vapor pressure of a component in a mixture is equal to the vapor pressure of the pure component at that temperature multiplied by its mole fraction in the mixture. ... The total vapor pressure of the mixture is equal to the sum of the individual partial pressures
first, find the mole fractions.
Moles of benzene, moles toluene. Then, add to get total moles
Then, partial vp of toulene= .85*molestoulene/totalmoles
and same method to get vp of benzene.
Add the two partial vp to get total solution vp