If 11.5 g of CCl_3F is enclosed in a 1.2L container, will any liquid be present?

To determine whether any liquid will be present in the 1.2L container when 11.5g of CCl3F is enclosed, we need to compare the density of CCl3F with the density of the liquid state.

1. Start by finding the molar mass of CCl3F (carbon tetrachloride):

C = 12.01 g/mol
Cl = 35.45 g/mol
F = 18.99 g/mol

Molar mass of CCl3F = (3 x 35.45) + 12.01 + 18.99 = 137.33 g/mol

2. Determine the number of moles of CCl3F:

Number of moles = Mass / Molar mass
Number of moles = 11.5g / 137.33 g/mol

3. Calculate the density of CCl3F:

Density = Mass / Volume

Since we are given the mass but need to determine the volume, we rearrange the equation:

Volume = Mass / Density

Given:
Mass = 11.5g
Density = ? (unknown)

To find the density, we need the density value for CCl3F. Let's assume it is 1.6 g/mL for this example.

Density = 11.5g / (1.2L x 1,000mL/1L) = 9.58 g/mL

4. Compare the CCl3F density with the density of the liquid state:

If the density of CCl3F is less than the density of the liquid state, the substance will be in the gas phase.
If the density of CCl3F is greater than or equal to the density of the liquid state, the substance will be in the liquid phase.

Unfortunately, I don't have the density value for the liquid state you are referring to. Can you provide the density of the liquid you are asking about?