Essay On Inhomogeneous Liquid Bound In Nanopores

Whenever a monolayer is attached to a metal surface, the wetting properties and behavior can be significantly affected (Yuan & Lee, 15). In practice, densely-packed self-assembled monolayers (SAMs) can be used to modify the macroscopic properties of a solid surface (Dilimon et al. 202). Changes in wetting properties occur due to changes in the angle made by a liquid droplet whenever it is in contact with the surface. This phenomenon is significant in several contexts for example, in industrial contexts: this property is used to evaluate the cleanliness of semiconductor wafers. In such contexts, contact angles measurements are widely used. Control of this property is also useful during penetration of insecticides or pesticides into plants, and waterproofing of materials (Yuan & Lee, 25). While the former focuses on maximization of wetting, the latter case seeks to minimize liquid-induced wetting (Yuan & Lee, 28).

Of the two alkane liquids studied n-Hexane was determined to have the stronger IMF of attraction by virtue of its experimentally determined lower ?T. Conversely n-Pentane has weaker IMF of attraction due to its larger ?T. As explained at length above, this is because it takes more energy to excite a molecule in liquid to leave (vaporize or become gaseous), when there are stronger IMF of attraction holding the molecules together in liquid form.

In the experiment I performed it was proven that, the moles of a solute, the volume of the solvent, and the molarity of an aqueous solution share a mathematical relationship. Solutions, solutes and molarity are all terms that are crucial to chemistry. A solution is defined as a liquid mixture in which the solute is distributed into the major component, and a solute is defined as the minor component within a solution. The molarity of a solution is the number of moles of solute per liter of solution and it is used to express the concentration of a solution. Both the solute amount and the solution volume can be determined in experiments to aid finding the solution concentration or molarity of a substance that they are included in. I state confidently

Courtney Hofer Biology 1 Lesson 1.04 Properties of Water July 31, 2014 LAB REPORT Title: Drops on a Penny Hydrogen bonds and Surface tension gives water (H2O) some cool interesting properties, I am going to use these water properties to see how many drops of water and soap fit on a penny. Problem/Question: How many drops of water and soap fit on a penny?

Because water is polar, water can only ‘adhere’ to other polar substances. After the water on the penny has spilled over. On a molecular scale, the hydrogen bonds are being broken. After completing this experiment, we concluded that due to the amphipathic properties of the soap detergent, the penny would not be able to hold as many drops as a penny without the soap. Again, this is because soap is non-polar and in order for water (water is polar) to ‘mix’ with another substance, that other substance has to be polar as

so that the conductometric data were treated by Fuoss–Shedlovsky method [11] by using a computer program, to evaluate the ion-pair association constants of the studied salts and to re-evaluate the limiting molar conductance (Λ0), where they proposed the following equation:

The impact of the intermolecular forces: hydrogen-bonds, London Dispersion Forces, dipole-dipole attraction, and ion-dipole attraction were investigated in this lab, and it was determined that ion-dipole attraction results in the greatest amount of surface tension, followed by hydrogen-bonds, dipole-dipole attractions, and London Dispersion

The eluting solvent passed down the column by the gravity and an equilibrium was established between the solute absorbed by the absorbent (silica gel in this experiment) and the eluting solving flowing down. Since the components in the sample had different polarity and they interacted with the stationary phase and the mobile phase differently, the components would be carried by the solvent to a different extent and a separation of the components could be achieved.

In this lab, lab 4.3 Comparing the Concentrations of Saturated Solutions, we set out to find and compare the solubilities of two solids in water. In addition, we tested if solubility is a characteristic property of a solid in a given liquid. This lab allowed us to test and use a reliable way to measure the solubility of a solid. This lab can be replicated for any solid with the same procedure, thus it gives us a method to calculate solubility. The two solids we tested in this experiment were NaCl (Sodium Chloride) and NaNO3 (Sodium Nitrate).

In class, we are learning all about the properties of water. There are many properties of water including, cohesion, surface tension, adhesion, capillary reaction, polarity, high specific heat, and it is a universal solvent. During class, we did experiments to test these properties. The results proved all of them to be true.

Fig. 7 shows the plot of ln KC versus 1/T for the adsorption of Pb2+ ion onto the tested active carbon at the chemically simulated battery condition. The positive value of the calculated standard enthalpy (∆H◦), 2.62 kJ/ mol, indicates the endothermic nature of the uptake process. Furthermore, the process is entropy, and not enthalpy, driven due to the randomness increasing at the solid/ liquid interface during the adsorption process where the positive standard entropy change (∆S◦) is 0.011 kJ/ mol K

The objective of this experiment was to investigate the relationship of dispersion forces and hydrogen bonding forces in intermolecular attractions through the evaporation of different substances. Using temperature probes, the endothermic process of evaporation is measured by inserting the probes into the substance and then taking them out to allow the substance to evaporate, the change in temperature of the substances showed if a lot or not a lot of evaporation occurred and over how long the evaporation took place depending on if the change in temperature was high or low.

Osmosis is the “diffusion of water across a selectively permeable membrane” (Raven et al. G-16). In this experiment, dialysis tubing was used to mimic the selectively permeable membrane to show what osmosis does when placed in different solute concentrations. We filled the dialysis tubes with different percentages of solute and placed them in beakers full of another percentage of solute. Through this experiment, I saw what happens when the tube becomes hypertonic, hypotonic, and isotonic. “If two solutions have unequal osmotic concentrations, the solution with the higher concentration is hypertonic, and the solution with lower concentration is hypotonic.” (Raven et al. 98) “When two solutions have the same osmotic concentration, the solutions are isotonic.” (Raven et al. 98) My hypothesis was that the bags placed in hypertonic solutions would shrink because the water would leave the bag to go to the higher concentration. The bags placed in isotonic solutions would stay the same weight because the water would be going in and out evenly. The bags placed in hypotonic solutions would swell because water would rush into the cell where the higher concentration was. If bag A shrinks then it is hypertonic. If bag B stays the same, then it is isotonic. If bag C and D swell, then they are hypotonic.

The cheapest solvent is water, which possesses many physico-chemical properties. It can dissolve ionic components and form highly conducting solutions. Water, deionized and repeatedly distilled with alkaline KMnO4, is usually considered as pure. The purity is checked by conductivity measurements. The volatile and organic impurities [36] are removed by passing the distilled water vapour through a column containing Pt catalyst at about 800C over which oxygen also simultaneously passed.

One of the original and still most active fields of research in metal-organic frameworks is in gas separation. While the ability of both rigid and flexible MOFs to adsorb is based on such factors as geometry of the gas as well as sorbate-sorbent interactions, flexible MOFs are also dependent on structural rearrangements and the ability of the pore to change with thermodynamic conditions. Currently, most MOF investigations into gas separation are conducted by measuring the sorption and desorption of specific gases and relating isothermic data. MOFs are being looked to as next generation gaseous adsorbent materials in both industrial and environmental applications.9