Synthesis Reaction Lab Report

The purpose of this lab is to determine the formula of an unknown hydrate. To achieve this, we heated a hydrate over a Bunsen burner to drive out the water. As a result, the anhydrate is left and the data is used to calculate the mole ratio between the amount of anhydride and water. Then the mole ratios are used to calculate the hydration number, which was 4.8, but was rounded to 5 in the formula. The accepted formula is 〖CuSO〗_4∙5H_2 O and the percent of error was 4%.

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

In this experiment, we learned about stoichiometry, empirical formula, molecular formula, polyprotic acids and bases, metathesis reactions, and moles.

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.

3. Find the number of atoms of each of the substances involved in the reaction.

The percent of water can be determined in a hydrate by first determining the mass of the hydrate Copper (II) Sulfate penta-hydrate. The substance will be a deep blue color when it is a hydrate. By heating the substance, water is evaporated, removing the water from the hydrate, making it anyhydrous through a simple decomposition reaction. Evaporation is completed when the substance turns from a blue to a white/ grey color. The mass of the water in a hydrate is determined by subtracting the mass of the hydrate from the mass of the anhydrate. The mass of the water is then divided by the mass of the hydrate, and multiplied by one hundred, resulting in the percent of water in the hydrate, which is 36.35%. The percent error is determined by subtracting

Please Note: This lab involves a lot of waiting for the gas collection. Make sure you allot yourself the full three hours to perform the experiments.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

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

The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

3) Repeat the drying process just to be sure that the copper is completely dry, and again determine the mass of the copper and the beaker.

The malachite basic copper carbonate formed as CuCO3 ⋅ Cu(OH)2 shows bright green, whereas that of azurite formed as 2CuCO3 ⋅ Cu(OH)2 shows strong blue. In this study, most of the manufactured copper carbonate was converted to malachite basic copper carbonate of bright green at the reaction mole ratio of >1.20. In the case of low reaction ratio of sodium carbonate, m, the stoichiometric coefficients of CuCO3, is higher than n, the stoichiometric coefficient of Cu(OH)2, so that the amount of CuCO3 is generated is more than that of Cu(OH)2. With increasing reaction mole ratio of sodium carbonate, m is lower than n so that the generation rate of CuCO_3 is lower than that of Cu〖(OH)〗_2. Therefore, copper content increased with increasing sodium carbonate. With assumption of same value of m and n, theoretical copper content becomes 57.5