The most common phase transition to ice Ih occurs when liquid water is cooled below 0°C. As a naturally occurring crystalline solid with an ordered structure, ice is considered a mineral. It possesses a regular crystalline structure based on the molecule of water, which consists of a single oxygen atom covalently bonded to two hydrogen atoms, or H-O-H. Many of the physical properties of water and ice are controlled by the formation of hydrogen bonds between adjacent oxygen and hydrogen atoms. It is a weak bond, but is decisive in controlling the structure of both water and ice.
With a density of density 0.89990 g/liter. The freezing point of neon is -248.67° C, and the boiling point of neon is -246.048° C, which is even lower than the boiling point of nitrogen (-195.8°C). When under low pressure, neon emits a bright orange-red glow if a small electric current is passed through it. The electron configuration of neon is 1s22s22p6. The chemical properties of neon include the fact that it is not reactive because it has a full outer shell, and therefore cannot gain or lose any electrons.
The Empirical Formula of an Oxide, Purpose: The purpose of this lab was to determine the empirical formula of magnesium oxide. To do this, we measured the weight of the magnesium before the reaction with oxygen, and then measure it after it had bonded with the oxygen. After the mass of the items were collected, the data was calculated in empirical formula. Background: The empirical formula of a compound is the whole number ratio of the elements in a compound. For example, the empirical formula of water is H2O meaning for every 1 O atom there are 2 H atoms.
The formula containing the lowest possible ratio is known as its simplest formula ; also called the empirical formula. To find the simplest formula of a compound one can carry out an experiment of determining the mass of the compound, then the moles, hence the ratio. Objective The objective of this experiment was to prepare a compound and collect data from which you can determine the mass of each element in the compound. From the mass of each element in a compound, determine its simplest formula. In this case, the simplest formula of Magnesium Oxide.
Thermodynamics and Kinetics of Carbonates 3/31/2014 Experimentally it was determined that with the presence of magnesium in solution, aragonite readily transforms to calcite. By analyzing the data collected by Group 7 (Friday Lab 2) it can be concluded that the presence of magnesium acts as an inhibitor for the aragonite – magnesium transformation. 1.0 Introduction The objective of this lab is to practically apply knowledge of thermodynamics and kinetics. A stronger understand of X-Ray Diffraction (XRD) measurements will also be gained. Laboratory 2/3 will follow the rate at which aragonite transforms to calcite.
Titration Lab Period 3 5/20/12 Objective: The main objective of this lab was to determine the amount of sodium hydroxide needed to neutralize 10 milliliters of hydrochloric acid. We also had to calculate the molarity of the sodium hydroxide using our data. Concepts: Some different concepts used in this lab: indicators, titration formula, titration curves, pH levels, acids, and bases. Materials: Materials used in this lab: a 250mL beaker, ring stand, burette, Erlenmeyer flask, stop cock, burette clamp, 10mL HCL, 10mL NaOH, 3 drops of phenolphthalein, and pH paper. Procedure: 1.
W = Wa + 1.06 Wa/1000 Table. Density of water at various temperatures. Temperature (°C ) 26 27 28 29 30 31 32 33 34 Density of water ( g mL-1) 0.99681 0.99654 0.99626 0.99597 0.99567 0.99537 0.99503 0.99473 0.99440 How to use a pipette 1 Rinse a 25-mL pipette with two or three small volumes of distilled water, and then with a complete volume of distilled water. 2 Do not immerse the tip of the pipette too deep into the water. The tip should not be above the water level so as to avoid any mishap during the suction of the water into the pipette via the pipette filler or suction bulb.
Then you will fill a BURETTE with sodium hydroxide (a base) that has a known concentration. Because all the reactants and products in this reaction are colourless, an INDICATOR DYE is added to the sulphuric acid to let us know when all the acid present has been EXACTLY NEUTRALIZED by adding base. Finally, the sodium hydroxide in the burette is added to the acid/indicator solution until the indicator changes colour. (An indicator dye is a chemical that has a different colour in an acid and a base.) PROCEDURE 1.
c) 0.08 g of oxygen reacted with the magnesium (0.22 g – 0.14 g = 0.08 g). d) Refer to “Determining the Empirical Formula of Magnesium Oxide Lab Solutions” sheet e) Element | % | m (g) | M (g/mol) | n (m÷M) | ÷ by | Ratio | Magnesium | 63.63 | 63.63 | 24.31 | 2.617441382 | 2.273125 | 1 | Oxygen | 36.37 | 36.37 | 16.00 | 2.273125 | 2.273125 | 1 | Since the ratio is 1:1, the empirical formula is MgO. 2. Refer to “Determining the Empirical Formula of Magnesium Oxide Lab Solutions” sheet 3. You need to round the empirical formula to a whole number ratio because you cannot have decimals in the subscripts, which means that you cannot have a fractional amount of molecules in a substance.