hydrate before heating .9989g Weight hydrate after heating .6534g Weight of water .3455g Mole of water in hydrate .0192mol Mole of anhydrous salt: CuSO4 .004094mol CuCl2 .004859mol CoCl2 .005033mol Mole ratio of water to each of the anhydrous salts: CuSO4 4.69 CuCl2 3.95
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the mass of the hydrate and crucible gives the mass of the CuSO4 hydrate. Mass of hydrate = (mass of crucible + hydrate) - (mass of empty crucible) Mass of hydrate = (20.000g) – (15.000g) Mass of hydrate = 5.000g 2. Heat the hydrate. After heating‚ record the mass of the crucible and the dehydrated compound. No calculations for this step 3. Subtracting the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 gives you the mass of the dehydrated compound. Mass of dehydrate
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precipitate‚ or the evolution of heat are associated with a chemical change; to study reactions of copper. Copper is an element that can be found in nature in a variety of different compounds. The most common natural ore is the sulphide‚ known as chalcocite‚ Cu2S. This mineral is an important source of copper metal because it is about 80% copper by weight. Copper has many important uses due to its chemical and physical properties. Copper is a good conductor of both heat and electricity‚ hence it can
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scientists inadvertently produce undesired products that must be filtered or decanted out of solution (Petrucci et al‚ 2007). Beginning with pure copper wire‚ this experiment will exhibit its transformation to substances including Cu(NO3)2‚ Cu(OH)2‚ CuO‚ CuSO4 . 5H2O and finally returning to pure copper (Cu). The experiment objective is to successfully complete these conversions and then calculate the percentage of recovered copper using the initial and final mass data obtained. Procedure Please refer
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form the bonds of the products is greater than the energy required to break the bonds of the reactants. In an exothermic reaction‚ heat is given off to the surroundings; thus‚ temperature of the surroundings will increase. By measuring the change in the temperature and using the formula Q= mcΔT‚ we can calculate the enthalpy change of the reaction. Equation 1: CuSO4 + Zn ZnSO4 Ionic Equation: Zn (s) + Cu2+ (aq) Cu (s) + Zn2+ (aq) MATERIALS/APPARATUS: * 1 insulated Styrofoam cup
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Determining the Formula of a Hydrate Purpose: To determine the formula of a hydrate. Materials: * crucible * Bunsen burner * balance * CuSO4 hydrate Procedure: 1. Measure the mass of the clean‚ empty crucible‚ record the mass. 2. Add one or two scoops of the hydrate to the crucible‚ record the mass. 3. Heat the crucible and hydrate above a Bunsen burner for at least ten minutes to make sure that all of the water evaporates. 4. Let the crucible cool and then
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white in just 1 minute. In other words‚ there is an uneven heat distribution‚ which give rises to inconsistent colour of the hydrated salt (i.e. there were a few white speck and the rest is still blue). Moreover‚ some of the hydrated salt also spattered. In addition‚ at the end of the heating process‚ the finer grains were also turned to light yellowish-green. Processed Data Calculation needed: In order to find ‘’ in the formula CuSO4.H2O‚ we need to find the ratio of mole between anhydrous copper
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Reactions Chemistry Department UCC 1st Year Practicals Introduction n n n n n Copper is one of the most important metals. Copper is reddish with a bright metallic lustre It is malleable‚ ductile‚ and a good conductor of heat and electricity (second only to silver in electrical conductivity) Its alloys‚ brass and bronze‚ are very important Has various oxidation states: 0 in elemental copper‚ +1‚ and +2 which is observable in corroded brass/bronze Oxidation states
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EXPERIMENT 2 Stoichiometry Introduction Stoichiometry is the study of the quantitative relationships in chemical reactions. By studying stoichiometry‚ you can calculate the quantity of reactants that will be consumed in a chemical reaction‚ and the amount of product produced. Consider the reaction of vinegar with baking soda. As you may know‚ this reaction produces carbon dioxide gas which bubbles out of the vinegar. But if you want to know how much gas would be produced from combining a teaspoon
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water molecule with the sodium chloride dissolved in it with the carbon dioxide gas bubbles. 4. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) Na+ + OH- + H+ + Cl- → Na+ + Cl- + H2O(l) OH- + H+ → H2O This reaction with a strong acid‚ as noted‚ released heat‚ which we call an exothermic reaction. 5. BaCl2(aq) + H2SO4 → BaSO4(s) + 2HCl Ba+2 + 2Cl- + 2H+ + SO4-2 → BaSO4(s) + 2H+ + 2Cl- Ba+2 + SO4-2 → BaSO4(s) Here we have Hydrogen and chlorine as spectator ions. One of the solubility rules is that sulfates
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