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Oxidation-Reduction Reaction Lab

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Introduction An oxidation-reduction reaction involves transferring electrons in a chemical reaction. In a redox reaction, there are oxidizing agents that gain electrons and cause other substances to lose electrons, and reducing agents that lose electrons and cause other substances to gain electrons. Oxidation-reduction reactions are applied in many real-life situations. These reactions are often found in electrochemical batteries, photosynthesis and the burning of fossil fuels.1 Objective For our lab, we paired specific metals to different metal ions to determine which reactions would occur and therefore which were the best reducing/oxidation agents. We then preformed a second experiment using sodium iodide in three different reactions with …show more content…

For our mixtures, we placed the metal pieces inside of a small test tube, poured 1-2 mL of the metal ion solution into the tube, waited 30 minutes, and decided if there was a reaction or not. For the second experiment, we dissolved 0.5 g of solid copper(II)nitrate in 20 mL of deionized water and 0.5 g of sodium iodide in a separate 20 mL of deionized water, combined the two solutions, and recorded our observations. Then we combined 2 mL of 0.1 M sodium iodide, 2 mL hexane, and 2 mL of iron(III)chloride in a test tube and recorded our observations. Lastly, we mixed 2 mL of 0.1 M sodium iodide, 2 mL hexane, and 2 mL of 0.1 M tin(IV)chloride in a test tube and recorded our …show more content…

We know this because the copper went from Cu2+ to Cu1+. From this reaction we can also write a balanced equation. 2Cu(NO3)2 + 4NaI 2CuI + I2 + 4NaNO3 Then we created a net ionic equation for the reaction. 2Cu2+(aq) + 4I- (aq) 2Cu+ + I20 With the reactants NaI + FeCl3, we can predict that Fe3+ is being reduced by I-. We know this because the iron went from Fe3+ to Fe2+. From this reaction we wrote a balanced equation. 6NaI + 2FeCl3 6NaCl + I2+ 2FeI Then we created a net ionic equation for the reaction. 2Fe3+ (aq) + 2I- (aq) 2Fe2+ + I20 Lastly with the reactants NaI + SnCl4, we predicted that Sn4+ is being reduced by I-. We predicted this because the tin went from Sn4+ to Sn2+. From this reaction we wrote a balanced equation. SnCl4 + 2NaI SnCl2 + I2 + 2NaCl Then we created a net ionic equation for the reaction. Sn4+ (aq) + 2I- Sn2+ + I20 When looking at a table of reduction potentials, some of the oxidation states did not match with our resulting metal cations. Fe3+ had a much higher electrode potential than iodine, even though we had predicted that it would be the opposite. Error could have resulted from incorrect equations for the three reactions in experiment

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While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

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An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

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The purpose of this experiment was to learn about metal hydride reduction reactions. Therefore, the sodium borohydride reduction of the ketone, 9-fluorenone was performed to yield the secondary alcohol, 9-fluorenol. Reduction of an organic molecule usually corresponds to decreasing its oxygen content or increasing its hydrogen content. In order to achieve such a chemical change, sodium borohydride (NaBH4) is used as a reducing agent. There are other metal hydrides used in the reduction of carbonyl groups such as lithium aluminum hydride (LiAlH4).

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Qualitative Data: Prior to combining the solution CuCl2 was a transparent blue and Na2CO3 was clear While combining the solutions CuCl2 and Na2CO3, the solution became a cloudy blue After filtering the a dry blue powder was left inside the filter paper and a clear solution had drained through the paper filter. Calculations: Molar Mass and Number of Moles of Reactants CuCl2 and Na2CO3 Molar Mass of CuCl2 = 63.55 g Cu + (2 35.45g Cl) Molar Mass of CuCl2 = 134.45g CuCl2 Molar Mass of Na2CO3 = (2 22.99g Na) + (3 16.00g O) + 12.01g C Molar Mass of Na2CO3 = 105.99g Na2CO3 Moles of CuCl2 = Mass of CuC =

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Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.

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For Station 4 , the magnesium and zinc turnings blackened when introduced to Cu(NO3)2 . Copper (II) nitrate, zinc nitrate and magnesium nitrate all changed colour when sodium carbonate was added. b)Magnesium is most reactive (#1). Zinc is second most reactive (#2). Copper is the least reactive (#3).

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Cu(s) The flow of electrons will move from zinc ( anode electrolytic cell) to copper (cathode electrolytic cell). The overall reaction looks like

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As soon as the wire was submerged into the solution, the aluminum atoms and the copper (II) ions underwent a reduction-oxidation (redox) reaction, meaning aluminum was oxidized and donated its electrons to the copper ions, which were reduced. As a result, solid copper began to form on the surface of the aluminum wire, giving the wire a brown-orange color that resembled rust. The wire had to be regularly shaken in order to remove the solid copper particles and thereby expose more of the aluminum wire to react with the surrounding solution. As the reaction progressed, the liquid copper chloride solution slowly began to lose its color and turn clear. This was a chemical reaction, as seen by the bubbles formed with the wire was added, meaning gas was released when aluminum was oxidized and copper was reduced, but it also gave rise to physical changes, such as the change in color of the solution from blue-green to rusty orange to clear.

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In definition, an oxidation reaction is when any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. A weathered layer of copper oxide covers Lady Liberty that weighs about eighty tons. The color from brown to green only took thirty-four years after the statues construction, according to the New York Historical

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+ H2O (g) Reaction 4: when a sulphuric acid is added to the solution that contains copper (II) oxide, a double displacement reaction will occur. the copper (II) oxide will react with the sulphuric acid producing copper (II) sulfate and water. The copper and hydrogen gas replace each other. Balanced Chemical Equation: CuO (s) + H2SO4 (aq) —> CuSO4 (aq) + H2O (l) Reaction 5: when zinc is added to the copper (II) sulfate solution, a single displacement reaction will occur.

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In this experiment, a balanced chemical equation will be provided for decomposition reactions. A redox reaction is a reaction where one reactant is reduced due to a gain of electrons, and the other is oxidized due to a loss of electrons. The reactant that loses an electron is called the reducing agent, whereas the reactant that gains an electron is called the oxidizing agent. In this experiment, the balanced chemical equation, and the two half equations for the redox reactions will be provided, and the oxidizing and reducing agents will be

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The anode and cathode are related to the redox reaction because as copper ions move from the anode to the cathode the anode loses mass as the cathode gains mass. The anode and cathode losing and gaining mass is oxidation and reduction, as it is happening at the same time it is a redox reaction. An ionic equation for how redox reaction is related to anode and cathode

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Afterwards, 0.1ml of ferroin solution (as an indicator) was added. Next, titration was performed. The contents in the conical flask was titrated with 0.1M ammonia cerium (IV) sulphate until a yellow solution was produced. The experiment was then repeated without sample B (only the H2SO4 and water in the proportion 3:7, 6ml acid 14ml

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Copper is mainly used due to its better resistance in corrosion than other metals and its unwillingly nonreaction with most strong acids. To investigate and identify the nature of the reactions of copper, one can synthesize copper into a series of chemical reactions and explore its physical and chemical properties. The pure substance undergoing the chemical reaction, in this instant copper, takes on different chemical reactions. There are four types of chemical reactions: combination or synthesis reactions, decomposition reactions, substitution or single replacement

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In this experiment, the ions that go through gravimetric analysis are the copper and sulfate ions (Grossie and Underwood, 25). Elemental analysis involves determining the amount, which is usually a percent, of an element present in a compound (Blauch, 1). In this experiment, the element going through the elemental process hydrogen, in which the percent of the compound is attempted to be found (Grossie and Underwood, 25). In order to find the amount of copper, copper oxine needs to be formed. To find it, there is a reaction of hydrated copper sulfate and oxine, producing copper (II) oxine (Grossie and Underwood, 25).

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