To determine the heat of vaporization of nitrogen, we can use the Clausius-Clapeyron equation:
ln(P2/P1) = -(ΔHvap/R)(1/T2 - 1/T1)
Where:
P1 and P2 are the initial and final pressures, respectively.
T1 and T2 are the initial and final temperatures, respectively.
ΔHvap is the heat of vaporization we want to calculate.
R is the gas constant (8.314 J/(mol·K)).
Let's calculate the heat of vaporization (ΔHvap) using the given data:
P1 = 130.5 torr
T1 = 65 K
P2 = 289.5 torr
T2 = 70 K
First, convert the pressures from torr to atm:
P1 = 130.5 torr / 760 torr/atm
P2 = 289.5 torr / 760 torr/atm
Substitute these values into the equation:
ln(P2/P1) = -(ΔHvap/R)(1/T2 - 1/T1)
Solve for ΔHvap:
ΔHvap = -(R * (ln(P2/P1))/(1/T2 - 1/T1))
Repeat this process for each set of data to calculate the heat of vaporization at different temperatures and pressures.
Remember to convert all temperatures to Kelvin before performing any calculations.