Super Wooling Liquid Research

The objective of the experiment “Keeping it Liquid” was to figure out what it takes to keep a compound in a liquid form which caused a phase change. A phase change is when a substance changes from one state or phase to another. There are three main phases that normally occur and they are called Evaporation, Deposition, and Melting. Evaporation is where a liquid changes to a gas. An example of evaporation is when water drops form on the glass of a cold drink on a warm day. Deposition is where a gas vapor goes directly into the solid phase without becoming a liquid first. An example of Deposition often occurs on windows during the winter months. While Melting is where a solid turns into a liquid. Melting occurs when ice turn into a liquid when

3. Do you think sugar or salt will melt at a higher temperature? Explain your answer.

Other substances that dissolve in water also lower the freezing point of the solution. The amount by which the freezing point is lowered depends only on the number of molecules dissolved, not on their chemical nature. This is an example of a colligative property. In this project, you'll investigate different substances to see how they affect the rate at which ice cubes melt. You'll test substances that dissolve in water (i.e., soluble substances), like salt and sugar, as well as substances that don't dissolve in water (i.e., insoluble substances), like sand and pepper. Which substances will speed up the melting of the ice?

These resulting differences have a direct consequence on the solvation properties of SCW. Ionic association occurs to a larger extent in SCW because of the lower solubility of ions in water under extreme conditions. Aqueous electrolyte solutions constitute an integral part of a large number of biological and geological processes. Particularly, the thermodynamic properties of ions in supercritical water (SCW) have crucial roles in many geological processes [13]. Therefore, it is important to study and model the solvation structure and dynamics of aqueous electrolyte solutions in supercritical conditions at the microscopic level for the purpose of understanding the chemical processes and properties of such hydrothermal systems. Ion hydration and ion-pair association in SCW have been the important subjects for hydrothermal technologies [14]. Aqueous fluids which occur ubiquitously in the earth’s crust and upper mantle at higher temperatures and pressures are involved in magmatic processes, metamorphism,

The response earned a final point for the discussion of the ability of water to moderate temperature: water

The first part of the lab began by one lab member adding 10.0 mL of DI water to a test tube while another lab member obtained a beaker full of ice and salt. After both these steps were complete the test tube was put in the beaker full of ice. Immediately following the test tube be being placed in the beaker, a temperature probe was inserted into the test tube. The initial temperature was recorded and after the temperature was recorded in 30 second increments. Once the water exhibited supercooling and then remained consistent at .1 °C for 3 readings it was determined that the water had froze and formed crystals. Evidence that crystals formed allowed for it to be confirmed that the water actually hit freezing point at .0

Purpose: The purpose of this laboratory was to gain an understanding of the differences between the freezing points of pure solvent to that of a solvent in a solution with a nonvolatile solute, and to compare the two.

It’s predicted that when adding the chemical substance into the water, energy will be released or absorbed, this will be observed by a temperature change, therefore, there would be an exothermic or endothermic reaction.

The incorrect chemistry is that Olaf was in the water. This is incorrect because ice cannot be placed in warm water because it will acquire heat and turn from solid state to a liquid state. The heat is always transmitted from the hot body to the cold body. The hot body loses heat and the cold body acquires heat. Ice melts at 32 degrees Fahrenheit (0 degrees Celsius) During the transformation process, the temperature remains constant at 32 degrees Fahrenheit (0 degrees Celsius) until all ice is turned into water.

The fact that most small biological molecules dissolve in water is very important because all the chemical reactions that take place in cells do so in aqueous solution. Plants cam only obtain mineral salts in solution and human digestion will only dissolve soluble foods, meaning large starch molecules must be broken down into soluble sugars. Also many organisms living in water spend most of their time underwater, yet they require oxygen to respire, and as water is such a good solvent the required oxygen gas is dissolved in water. Water’s solvent properties also allow it to act as a transport medium for polar solutes for example the movement of minerals to lakes and seas and removal of metabolic wastes such as urea and ammonia in urine. Water’s thermal properties relate to its heat capacity.

Colligative properties, such as boiling point and freezing point, are dependent on the amount of solutes added, not necessarily their identities (LibreTexts, 2018). A fascinating concept related to freezing points is Supercooling. Supercooling is a state where liquids do not form ice even when they reach temperatures below their normal freezing point; they are trapped in a metastable state (Esrf.eu, 2018). The best example of this is clouds at high altitudes: they contain tiny droplets of water that do not have seed crystals, and therefore do not form ice despite the low temperatures (Esrf.eu, 2018). The concept of freezing point depression is applicable in many parts of everyday life.

Water is a covalent bond with one, negative charged, oxygen and two, positive charged, hydrogens. Water molecules, H20, are attracted to other water molecules forming a hydrogen bond. Since water is a polar molecule, it has a positive to negative attraction, meaning that the oxygen bonds with other hydrogen from different water molecules. As water freezes the oxygen molecules attract to hydrogen molecules and the hydrogen will begin to crystallize causing the water molecules to move farther apart. This is why ice is less dense than

Water a transparent and formless liquid that is one of the most important things that we have on planet Earth. Every living thing needs water to live, so it is considered to be the source of life, by many.

The purpose of this lab was to study colligative properties. These properties are properties that are affected when a solute is added to a solvent. Thus, the amount is important, not the actual type of substance, for the colligative properties. A couple types of this property are the freezing point and boiling point of a substance. (1)

These phases can go from one to another when affected by certain things, which is known as phase changes. To switch from a solid to a liquid, the solid must melt. On the other hand, to switch from a liquid to a solid, freezing must occur. Furthermore, to switch from a liquid to a gas, a process known as evaporation must take place. In contrast, to