Unit 3 Intermolecular Forces Lab
Khanya Ramey
Tuesday Nov. 24
Intermolecular Forces
Intermolecular Forces Lab
II. Goal:
The central goal of this experiment is to depict the intermolecular forces of four different properties of solubility, evaporation, viscosity, and boiling point.
The reason for achieving the goal is so we can further understand solubility, Evaporation, viscosity, and the boiling point of liquids. III. Experimental procedures
In this Lab there were four different stations to experiment with, my partner and I started with grabbing our goggles, and then we started with station 4, solubility, we had add a small amount of 4 different liquids (Hexane, Ethanol, Water, or Vegetable oil) to a well, then we had add a solid (Salt,Sugar, or Lard) to each of the 4 …show more content…
As with Lard none of the liquid dissolved with it. Adding the soap to the solids also didn’t dissolve anything. For the second station, Acetone had the lowest boiling point with 60 °C, then Hexane with 62 °C, Ethanol with 80 °C and lastly Water with the highest boiling point of 85 °C. For the third station, with the highest and lowest viscous, Hexan had the lowest viscous of 2.03, third was Ethanol with 1.39, second was Water with 1.33, and Mineral oil was the slowest with 1.09. For the fourth and final station, the liquid with the fastest evaporation time was Ethanol then last with the slowest evaporation times were water.
Evidence and analysis.
For station 1 water was the most soluble because it dissolved in almost all the solids and the other two liquids couldn’t. The water is soluble because the water when the solid is placed into it, it converts into a polar solvent molecule which then is able to liquefy the solid. For station 2, Ethanol is more viscous than any of the other solvent because it has a higher viscosity. In station 3, water boils the fastest because the molecules are moving so quickly in the glass
Tuesday Nov. 24
Intermolecular Forces
Intermolecular Forces Lab
II. Goal:
The central goal of this experiment is to depict the intermolecular forces of four different properties of solubility, evaporation, viscosity, and boiling point.
The reason for achieving the goal is so we can further understand solubility, Evaporation, viscosity, and the boiling point of liquids. III. Experimental procedures
In this Lab there were four different stations to experiment with, my partner and I started with grabbing our goggles, and then we started with station 4, solubility, we had add a small amount of 4 different liquids (Hexane, Ethanol, Water, or Vegetable oil) to a well, then we had add a solid (Salt,Sugar, or Lard) to each of the 4 …show more content…
As with Lard none of the liquid dissolved with it. Adding the soap to the solids also didn’t dissolve anything. For the second station, Acetone had the lowest boiling point with 60 °C, then Hexane with 62 °C, Ethanol with 80 °C and lastly Water with the highest boiling point of 85 °C. For the third station, with the highest and lowest viscous, Hexan had the lowest viscous of 2.03, third was Ethanol with 1.39, second was Water with 1.33, and Mineral oil was the slowest with 1.09. For the fourth and final station, the liquid with the fastest evaporation time was Ethanol then last with the slowest evaporation times were water.
Evidence and analysis.
For station 1 water was the most soluble because it dissolved in almost all the solids and the other two liquids couldn’t. The water is soluble because the water when the solid is placed into it, it converts into a polar solvent molecule which then is able to liquefy the solid. For station 2, Ethanol is more viscous than any of the other solvent because it has a higher viscosity. In station 3, water boils the fastest because the molecules are moving so quickly in the glass