The vapor pressure of CCl3F at 300K is 856torr. If 11.5g of CCl3F is enclosed in a 1L container, Will any liquid be present? If so, what mass of liquid?
If you use PV = nRT, plug in 856 torr for pressure (the vapor pressure of the liquid will be the pressure in the container if there is some liquid remaining) and solve for n.
Convert n to grams and subtract from 11.5
42
7.5
To determine whether any liquid will be present in the 1L container, we need to compare the vapor pressure of CCl3F at 300K to its actual vapor pressure. If the actual vapor pressure is less than 856 torr, then some liquid will be present.
To calculate the actual vapor pressure, we can use the ideal gas law equation: PV = nRT.
First, let's calculate the number of moles of CCl3F:
n = mass / molar mass
The molar mass of CCl3F can be calculated by adding up the atomic masses of carbon (C), chlorine (Cl), and fluorine (F):
Molar mass of CCl3F = (1 * atomic mass of C) + (3 * atomic mass of Cl) + (1 * atomic mass of F)
Next, calculate the actual vapor pressure using the ideal gas law:
PV = nRT
Here, P is the actual vapor pressure of CCl3F, V is the volume (1L), n is the number of moles of CCl3F, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature (300K).
Once we have the actual vapor pressure (P), we can compare it to the given vapor pressure (856 torr) to determine if there will be any liquid present.
If the actual vapor pressure is less than 856 torr, it means the actual vapor pressure is lower than the given vapor pressure. In this case, some liquid will be present.
To calculate the mass of the liquid, we can subtract the mass of the gas from the total mass:
Mass of liquid = Total mass - Mass of gas
Now, let's calculate the actual vapor pressure and determine if any liquid will be present:
1. Calculate the molar mass of CCl3F:
- Carbon (C) atomic mass = 12 g/mol
- Chlorine (Cl) atomic mass = 35.5 g/mol
- Fluorine (F) atomic mass = 19 g/mol
- Molar mass of CCl3F = (1 * 12) + (3 * 35.5) + (1 * 19) g/mol
2. Calculate the number of moles of CCl3F:
- Moles = mass / molar mass
3. Calculate the actual vapor pressure using the ideal gas law:
- PV = nRT
- P = (n * R * T) / V
4. Compare the actual vapor pressure with the given vapor pressure (856 torr).
5. If the actual vapor pressure is less than 856 torr, some liquid will be present.
6. Calculate the mass of the liquid:
- Mass of liquid = Total mass - Mass of gas
Applying these steps will provide the answer to the question and determine whether any liquid will be present in the 1L container, as well as the mass of the liquid if applicable.