A solution is prepared by mixing 50 g of methanol (CH₃OH) with 50 g of ethanol (CH₃CH₂OH). Use the following data to determine the vapor pressure of this solution at 20 $\circ$ C. A)69 torr B)57 torr C)80 torr D)73 torr E)83 torr

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Quizplus · Accepted Answer

To find the vapor pressure of the solution, we use Raoult's Law, which states that the vapor pressure of a solution is the sum of the vapor pressures of each component multiplied by their respective mole fractions. First, calculate the moles of methanol and ethanol:- Molar mass of methanol (CH3OH) = 32.04 g/mol- Molar mass of ethanol (C2H5OH) = 46.07 g/molMoles of methanol = 50 g / 32.04 g/mol = 1.56 molMoles of ethanol = 50 g / 46.07 g/mol = 1.09 molTotal moles = 1.56 mol + 1.09 mol = 2.65 molMole fraction of methanol = 1.56 mol / 2.65 mol = 0.589Mole fraction of ethanol = 1.09 mol / 2.65 mol = 0.411Using Raoult's Law:Vapor pressure of solution = (Mole fraction of methanol * Vapor pressure of methanol) + (Mole fraction of ethanol * Vapor pressure of ethanol)= (0.589 * 92 torr) + (0.411 * 45 torr)= 54.228 torr + 18.495 torr= 72.723 torrRounded to the nearest whole number, the vapor pressure of the solution is 73 torr.

A Solution Is Prepared by Mixing 50 G of Methanol ∘\circ∘

A Solution Is Prepared by Mixing 50 G of Methanol $\circ$