What is the pressure of an ideal solution containing .5 moles of a nonvolatile solute and 300g of ethanol at 40C? The vapor pressure of ethanol is 134 torr at 40C

The pressure of the solution is 144 torr

Explanation:

Step 1: Data given

Number of moles of a nonvolatile solute = 0.5 moles

Mass of ethanol = 300 grams

Molar mass of ethanol = 46.07 g/mol

Temperature = 40°C

The vapor pressure of ethanol = 134 torr

Step 2: Calculate moles ethanol

Moles ethanol = mass ethanol / molar mass ethanol

Moles ethanol = 300 grams / 46.07 g/mol

Moles ethanol = 6.51 moles

Step 3: Calculate the total moles

Total moles = 0.5 moles + 6.51 moles

Total moles = 7.01 moles

Step 4: Calculate mol fraction

Mol fraction = moles / total moles

Mol fraction ethanol = 6.51 / 7.01 moles

Mol fraction ethanol = 0.93

Mol fraction nonvolatile solute

0.5 moles / 7.01 moles = 0.07

Step 5: Calculate Total pressure of the solution

Vapor pressure ethanol = mol fraction * total pressure solution

134 torr = 0.93 * total pressure solution

Total pressure solution = 134 torr/ 0.93

Total pressure solution = 144 torr

The pressure of the solution is 144 torr

h let me think

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