Question

At a certain temperature the vapor pressure of pure thiopene (C4H4S) is measured to be 0.56 atm. Suppose a solution is prepared by mixing 123 g of thiopene and 137 g heptane (C7H16). What is the partial pressure of thiopene vapor above this solution?

Answer 1

Use Raoult's Law to determine the partial pressure of thiophene in the solution by calculating the mole fractions of thiophene and heptane and then applying the vapor pressure of pure thiophene.

Step-by-step explanation:

To find the partial pressure of thiophene vapor above the solution, we use Raoult's Law, which states that the vapor pressure of a component in an ideal solution is directly proportional to the mole fraction of the component in the solution times the vapor pressure of the pure component.

First, we calculate the moles of thiophene and heptane using their molecular weights (C4H4S = 84.14 g/mol and C7H16 = 100.2 g/mol) and the given masses (123 g of thiophene and 137 g of heptane).