The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of chloroform.
Chloroform=119.40
I do not know how to start this. Thank you for your help!
Convert g to moles for both solute and solvent.
Convert moles solvent to mole fraction solvent, Xchlor
Then Pchlor = Xchlo*PoCHCl3
To calculate the vapor pressure of the solution, we need to use Raoult's Law, which states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent in the solution.
First, we need to determine the number of moles of chloroform and aspirin in the solution.
Number of moles of chloroform:
molar mass of chloroform = 119.4 g/mol
mass of chloroform = 244.5 g
moles of chloroform = mass of chloroform / molar mass of chloroform
= 244.5 g / 119.4 g/mol
Number of moles of aspirin:
molar mass of aspirin = 180.1 g/mol
mass of aspirin = 6.243 g
moles of aspirin = mass of aspirin / molar mass of aspirin
= 6.243 g / 180.1 g/mol
Now, let's calculate the mole fraction of chloroform:
mole fraction of chloroform = moles of chloroform / (moles of chloroform + moles of aspirin)
Next, we need to calculate the vapor pressure of the solution using Raoult's Law equation:
vapor pressure of the solution = mole fraction of chloroform * vapor pressure of pure chloroform
Given that the vapor pressure of pure chloroform is 173.11 mmHg, we can now calculate the vapor pressure of the solution by substituting the values into the equation.