selenium tetrafluoride, SeF4 is a colorless. it has vapor pressure of 757mmhg at 105 deg c and 522mmhg a 95 deg c. what is the vapor pressure of carbon disulfide at 35 deg c?
You are switching from SeF4 to CS2. Are you using Trouton's Rule?
To find the vapor pressure of carbon disulfide (CS2) at 35 degrees Celsius, we need to use the information provided about the vapor pressure of selenium tetrafluoride (SeF4) at different temperatures.
Given:
1. Vapor pressure of SeF4 at 105 degrees Celsius: 757 mmHg
2. Vapor pressure of SeF4 at 95 degrees Celsius: 522 mmHg
To determine the vapor pressure of CS2 at 35 degrees Celsius, we can use the Clausius-Clapeyron equation, which relates the vapor pressure of a substance at different temperatures. The equation is as follows:
ln(P1/P2) = ∆Hvap/R * (1/T2 - 1/T1)
where:
P1 = Vapor pressure at temperature T1
P2 = Vapor pressure at temperature T2
∆Hvap = Heat of vaporization
R = Ideal gas constant (8.314 J/(mol∙K))
T1 and T2 = Temperatures in Kelvin
First, we need to convert the temperatures provided into Kelvin:
35 degrees Celsius + 273.15 = 308.15 K
Now, we can rearrange the Clausius-Clapeyron equation to solve for the vapor pressure of CS2 at 35 degrees Celsius (P2):
ln(P2/522 mmHg) = (∆Hvap/R) * (1/308.15 K - 1/368.15 K)
To solve the equation, we need to know the heat of vaporization for CS2. The heat of vaporization (∆Hvap) is the amount of energy required to convert one mole of liquid to gas at constant temperature and pressure.
Unfortunately, the heat of vaporization for CS2 is not provided in the given information. Therefore, we cannot determine the vapor pressure of CS2 at 35 degrees Celsius without this additional data.
If you have the heat of vaporization of carbon disulfide (CS2), I can help you calculate the vapor pressure at 35 degrees Celsius.