When a student plotted ln [vapor pressure of a gas] vs. inverse Kelvin temperature, she obtained a straight line with a slope equal to -9.500 x 10^3 K.
According to the Clausius Clapeyron equation, Hvap is kJ/mol.
http://www.science.uwaterloo.ca/~cchieh/cact/c123/clausius.html
To determine the value of Hvap (the heat of vaporization) in kJ/mol using the Clausius-Clapeyron equation, we need more information. Specifically, we need to know the value of the gas constant (R) in the equation.
The Clausius-Clapeyron equation relates the natural logarithm (ln) of the vapor pressure (P) of a substance to its temperature (T) and the heat of vaporization (Hvap):
ln(P2/P1) = -Hvap/R * (1/T2 - 1/T1)
Where:
- P1 and P2 are the vapor pressures at temperatures T1 and T2, respectively.
- R is the gas constant (in J/mol•K).
- T1 and T2 are the temperatures in Kelvin.
Given that we have the slope of the straight line from the plot, we can use it to determine the value of -Hvap / R. However, without knowing the value of R, we cannot calculate the absolute value of Hvap.
Once we have the value of -Hvap / R, we can multiply it by R to obtain the value of Hvap. The value of R can be found in the literature or provided as part of the problem.
Therefore, to determine Hvap in kJ/mol, we need to know the value of R. Please provide that information so we can help you calculate Hvap.