SO4-2 + 2H2O OH- + 2H+ → 2H2O(l) Aqueous ammonia is ammonia in water. Aqueous ammonia reacts with sulfuric acid‚ which then forms the salt ammonium sulfate and water. This is a neutralization reaction. 7. CuSO4 + Zn(NO3)2 → Cu(NO3)2 + ZnSO4 Cu+2 + SO4-2 + Zn+2 + 2NO3- → Cu+2 + 2NO3- + Zn+2 + SO4-2 All are cancelled out as spectator ions‚ so as observed there was no reaction that took place. 8. Na2CO3 + CaCl2 → 2NaCl + CaCO3(s) 2Na+ + CO3-2 + Ca+2 + 2Cl- → 2Na+ + 2Cl- + CaCO3(s) Ca+2 + CO3-2
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Cu(s) + 4HNO3(aq) --- Cu(NO3)2(aq) + 2H2O(aq) + NO2(aq) 2. HNO3(aq) + NaOH(aq)--NaNO3(aq) + H20(l) 3. Cu(OH)2(s)--CuO(s) + H2O(l) 4. CuO(s) + H2SO4(aq)-- CuSO4(aq) +H2O(l) 5. CuSO4(aq) + Zn(s)-- ZnSO4(aq) + Cu(s) At the end of reaction number five we should have close to 100% of the copper we started out with. Result Original Mass of Cu=.452g Mass of Cycled Cu=2.483g 1. In the first reaction oxidation-reduction occurs there were a brown smoke has the Cu dissolves
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Solutions Purpose/ Hypothesis: The purpose of this lab was to clearly identify the reactivity of magnesium‚ zinc and copper. The metals reactivity will be exemplified as it will be tested with different solutions such as zinc sulfate (ZnSO4)‚ copper sulfate (CuSO4)‚ hydrochloric acid (HCL)‚ magnesium sulfate (Mg2SO4)‚ iron (II) sulfate (FeSO4) and tin (II) chloride (SnCl2). This will allow us in creating an activity series to visually see the reactivity when given single displacement reactions.
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measure the cell potential (E˚cell) between various 1.0 M aqueous reactant solutions‚ then using balanced half-cell rxns‚ calculate theoretical cell potential values and compare to experimental. Part B: Concentration Cell: Measure the cell potential of CuSO4 (aq) of two differing Molarities – one concentrated and one dilute- then use the Nernst equation to determine the theoretical cell potential ‚ comparing to experimental. Part C: Electrolytic Cells- use an external source of electricity to drive the
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n 0 Cu Transition metal – different oxidation states Cu0 elemental state Cu+1 Cu+2 most common Cu+3/ Cu+4 unusual oxidation - 2 electrons 2+ Cu reduction + 2 electrons 0 Cu Objectives n To observe a sequence of chemical reactions starting and finishing in elemental copper metal‚ and to practice quantitative laboratory techniques. Cu → Cu(NO3)2 → Cu(OH)2 → CuO → CuSO4 → Cu Cu(NO3)2 = copper nitrate Cu(OH)2 = copper hydroxide CuSO4 = copper sulfate
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heat generated by the reaction is 55.8 kJ. The sign of T of the reaction used for calibration is opposite to that of H. In the determination of heats of reaction‚ the reaction of 15 mL 1 M CuSO4 + 0.05 g Zn produced a net ionic equation of CuSO4 + Zn ZnSO4 + Cu. The limiting reactant of the reaction is Zn and 0.05 moles of it was used. The sign of T of the reaction used for calibration is opposite to that of H. WORKING EQUATIONS: H+(aq) + OH-(aq) H2O(l) Hrxn= -55
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CHEMICAL REACTIONS OF COPPER AND PERCENT YIELD Objective To gain familiarity with basic laboratory procedures‚ some chemistry of a typical transition element‚ and the concept of percent yield. Apparatus and Chemicals |0.5 g piece of no. 16 or no. 18 copper wire |evaporating dish | |250 mL beaker (2) |weighing paper | |concentrated HNO3 (4 – 6 mL)
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Copper Cycle Summary During the copper cycle lab‚ my partners and I performed a series of reactions on copper powder and observed the changes it underwent. For the first step‚ we mixed nitric acid and copper powder‚ and noticed that a yellowish brown gas emerged‚ along with effervescence. The red solid disappeared and became a blue liquid. We know that we produced copper nitrate‚ nitrate gas‚ and water because the only two blue solutions in “A New Language” are copper sulfate and copper nitrate
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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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 to "Experiment
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