The vapor pressure of liquid chloroform, CHCl3, is 400.0 torr at 24.1 degrees Celsius and 100.0 torr at -6.3 degrees Celsius. What is delta Hvap of chloroform?

Use the Arrhenius equation.

I attempted using the Clausius-Clapeyron Equation and I am not getting anywhere

The cc should work. And I should have said cc instead of A. Are you using Kelvin for temperature. That is a common error. And 8.314 for R?

Ok I will try Kelvin. Thank you

To find the enthalpy of vaporization (delta Hvap) of chloroform (CHCl3), we can use the Clausius-Clapeyron equation. The equation relates the vapor pressures of a substance at two different temperatures to the enthalpy of vaporization.

The Clausius-Clapeyron equation is given by:
ln(P2/P1) = (delta Hvap / R) * (1/T1 - 1/T2)

Where:
P1 and P2 are the vapor pressures at temperatures T1 and T2 respectively
delta Hvap is the enthalpy of vaporization
R is the ideal gas constant (8.314 J/(mol·K))
ln denotes the natural logarithm

Given that the vapor pressure of chloroform is 400.0 torr at 24.1 degrees Celsius (T1) and 100.0 torr at -6.3 degrees Celsius (T2), we can rewrite the equation as:
ln(100.0/400.0) = (delta Hvap / R) * (1/(-6.3 + 273.15) - 1/(24.1 + 273.15))

Let's calculate the values of the equation step by step to find delta Hvap.

1. Convert temperatures from degrees Celsius to Kelvin:
T1 = 24.1 + 273.15 = 297.25 K
T2 = -6.3 + 273.15 = 266.85 K

2. Substitute the values into the equation:
ln(100.0/400.0) = (delta Hvap / R) * (1/266.85 - 1/297.25)

3. Solve for delta Hvap:
ln(0.25) = (delta Hvap / 8.314) * (0.00375 - 0.00336)

4. Simplify the equation:
ln(0.25) = (delta Hvap / 8.314) * 0.00039

5. Rearrange the equation to solve for delta Hvap:
delta Hvap = ln(0.25) * (8.314 / 0.00039)

Now, let's calculate the value of delta Hvap using the given equation.

delta Hvap = ln(0.25) * (8.314 / 0.00039)

Calculating this expression will give us the value of delta Hvap for chloroform.