Hydrate Lab Report for Chemistry Lab

If the hypothesis is correct, the masses after we place the tubing samples in water will be higher than the masses before. We will see the greatest % increase in mass in the highest concentration of sucrose (1.0 M). The % increase will get lower as concentration decreases. All of the samples should have some increase in mass because we are placing them in distilled water. Based on the known solutions, the data should yield a mathematical model relating concentration and % increase, which we can use to find the concentration of the unknown solution.

It used mass, temperature, length, volume, density, and making a dilute solution. I learned the importance as well as the difficulty of making proper measurements in a lab setting. If one measurement is off, it will throw the entire equation off. This will give either incorrect or inaccurate results.

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

4) If the masses agree, stop. If the masses are more than 0.05 gram different, then repeat the drying process until there is

We used a bunsen burner to burn the hydrate off and took the mass of the hydrate to make sure it was all gone.

Title: The relationship between the plant’s exposure to environmental conditions and the time it takes the chemicals to produce a reaction.

The lines in Figures 6 (A) to 6 (F) indicate predicted values, using fitted rate constants for the reaction. The rate constant valueswere found to increase as expected as the temperature was increased. The activation energies were determined from the temperature dependency of the rate constants to be 831, 2494, 3076 and 2660 J/molfor hydrazone, tryptophol, cinnoline derivative, and polyindole formation, respectively(Table 2). The values indicate the amount of energy required to cross the energy barrier so that,the reaction can takes place. The activation energy for hydrazone formation is low(Table 2) indicating that, the reaction takes place at lower temperatures buttheactivation energy barrier is higherfor tryptophol formation.

The occurrence of large natural clathrate hydrate deposits on the oceanic sea floors and the possibility that these gas hydrates could be mined as an energy source of hydrocarbon gas or used to sequester CO2 gas are still attracting considerable interest.

The objective of this investigation was to determine the chemical formula of the hydrate copper (II) sulfate. 3.4g of hydrate was grinded to a fine powder and afterwards heated at a medium setting on a hot plate until colour change from blue to a light grey occurred. Subsequently the colour change had occurred the mass of the hot anhydrous salt was measured to weigh 2.1g. The mass of the water evaporated was calculated to be 1.3g. After all the data was collected the percentage of water evaporated was calculated to be approximately 38%. The accepted stoichiometric ratio between copper sulfate and water was 1:5.

Determining the amount of Water of Crystallization Hydrated to Copper Sulphate Daniel Benda October 11th 2014 Hl Chemistry Block: H Word Count: 1354   Data Collection and Processing: Raw Data: Table 1: Raw data of Trials vs Mass of crucible and contents before and after heating Trials Empty mass of crucible (±0.001g) Initial filled mass of crucible (±0.001g) Final Filled weight of crucible (±0.001g) T1 36.093 43.516 40.783 T2 48.160 56.218 53.143 T3 31.503 44.537 39.705 T4 34.345 38.677 37.082 T5 33.615 41.851 38.787 Data for trial 1-3 were gathered by Jose and me while 4 and 5 were gathered by Ronnie and Michael Qualitative observations: As the hydrated salt is heated in the crucible it changes from a bright blue to a pale blue

Hydrazine is widely used in industrial and agricultural activities such as fuel cells, rocket propellants, explosives, antioxidants, corrosion inhibitor, insecticides and plant growth regulators.1,2 Although hydrazine possesses significant applications, it can raise potential threat to the living things because hydrazine is a toxic material which can be served as neurotoxin, carcinogenic and hepatoxic substance.3 Besides that, the exposure of high level of hydrazine can cause irritation to nose, eye, throat, dizziness, nausea, temporary blindness, pulmonary edema and coma, which will eventually endanger the liver, kidneys and central nervous system of humans.4

This lab demonstrated both the law of definite proportions and the law of conservation of mass. Because hydrates are compounds with a a constant composition and because the waters of hydration(water molecules bound to the salt crystals) can be relatively easily driven off by heating, the amount of water present in the hydrate can be

The process of hydrate nucleation both in natural and in techno genic conditions has a common basis when hydrates form from free water and gas. However, additional conditions which are determined by capillary pressure, surface tension, salt content of the fluid and capacitative properties of medium are applied during hydrate formation in a porous media. The formation of gas hydrate has to be categorised fewer than two groups 1) formation of hydrates from dissolved gas when the rate of hydrate accumulation is determined by the diffusive influx of gas from adjacent water and 2 from free gas contained in pores gas or gas condensate deposit transforms into gas hydrate one during a change in thermodynamic conditions. For the first case the molecules

The purpose of this lab is to determine the percent composition of water of the hydrate. Hydrates are solid ionic compounds that contain water that is chemically inside the crystalline structure. An example of such compound is epsom salt. A salt is an ionic compound that forms as a product of a reaction between both acid and base. Water molecules that are incorporated with salt are known as waters of hydration. The waters can be removed from the hydrate with the use of heat, thus, leaving the salt with no water molecules. The remaining amount of salt is referred to as anhydrous. An anhydrate is a substance that has been stripped of their water particles with the use of heat and has since become dehydrated. This experiment shows relevance to

The goal of this lab was to find the empirical formula of Magnesium sulfate hydrate. To determine this formula, we measured and recorded the mass of an empty clay crucible. We then poured a small amount of Epsom salt into the crucible, and then recorded the mass of the filled crucible. We then subtracted the weight of the empty crucible from the weight of the crucible with Epsom salt to determine the mass of the Epsom salt. We then lit a bunsen burner, and manipulated the airflow to allow for the optimal (hottest) flame. We then placed the bunsen burner under a clay triangle, suspended roughly 4 cm above the nozzle of the burner. Next, the crucible with the Epsom salt was placed on the triangle, and was heated by the bunsen burner for 8 minutes. After 8 minutes, the bunsen burner was turned off, and the crucible was set to cool for 5 minutes. After cooling, we measured and recorded the mass of the crucible. We then placed the crucible over the bunsen burner for 5 minutes, and then set it to cool for another 5 minutes. The mass of the crucible was then measured and recorded again.