🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.

Solution: Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities in water at 25 oC and 1 atm fluorocarbon pressure are given as mass percentages.FluorocarbonSolubility (mass %)CF40.0015CClF30.009CCl2F20.028CHClF20.30For CClF3, calculate the molality of a saturated solution.

Problem

Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 ^oC, and their solubilities in water at 25 ^oC and 1 atm fluorocarbon pressure are given as mass percentages.

Fluorocarbon	Solubility (mass %)
CF4	0.0015
CClF3	0.009
CCl2F2	0.028
CHClF2	0.30

For CClF₃, calculate the molality of a saturated solution.

Solution

We’re being asked to calculate the molality of ClF₃ given its solubility in mass percent.

Mass or weight percent (% by mass) is the percentage of a given element or compound within a solution. 

The equation used to calculate for mass percent is shown below:

$\boxed{\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}\mathbf{ }\mathbf{p}\mathbf{e}\mathbf{r}\mathbf{c}\mathbf{e}\mathbf{n}\mathbf{t}\mathbf{ }\mathbf{=}\mathbf{ }\frac{\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}\mathbf{ }\mathbf{c}\mathbf{o}\mathbf{m}\mathbf{p}\mathbf{o}\mathbf{n}\mathbf{e}\mathbf{n}\mathbf{t}}{\mathbf{t}\mathbf{o}\mathbf{t}\mathbf{a}\mathbf{l}\mathbf{ }\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}}\mathbf{\times }\mathbf{100}}$

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