I'm working on a problem dealing with calculating the heat of vaporization for vapor pressures problem.
By substituting the problems values into the Clausuis-Clapeyron equation I get:
.642= (2.28x10-5) x Delta H vap (J/mol)
However, from this point I don't know how to calculate a correct Delta H value?
It would be easier to help if you posted the complete problem along with the work you've done. If you're sure of what you've done to this point, the next step is
dHvap = 0.642/2.28E-5
To calculate the heat of vaporization (Delta H vap), you will need to rearrange the Clausius-Clapeyron equation and solve for Delta H vap. Here's how you can do it:
Step 1: Rearrange the equation. Divide both sides of the equation by the constant term (2.28x10^(-5)):
Delta H vap = .642 / (2.28x10^(-5))
Step 2: Perform the calculation.
Delta H vap = 2.81x10^(4) J/mol
Therefore, the heat of vaporization (Delta H vap) for your problem is 2.81x10^4 J/mol.
Keep in mind that the units should match throughout the calculation to ensure the accuracy of the result.