![]() ![]() ![]() Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.) Write the two equations which represent these reactions. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Solid iron reacts with Oxygen gas to form solid Iron (II) oxideĬopper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. _ C 3H 5N 3O 9 ® _ CO 2 + _ N 2 + _ H 2O + _ O 2Īqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide. (4 points) What are the signs given to the electrodes in both the voltaic and electrolytic cells? What reaction (oxidation or reduction) is occurring at each?īalance the following Chemical Equations: Be sure to mention the various parts of the voltaic cell and what they have to do with how it works.Ģ2. ( 5 points) Tell how a voltaic cell works. Write the oxidation numbers for both the reactants and the products ( 2 points) What is the reducing agent and why? ( 2 points)Ģ1. ( 5 points) Write the equation for the reaction of calcium and oxygen ( 1 point). Open response Questions : Answer questions 20 through 22 in complete sentencesĢ0. ¢ deposition of a salt layer on a metal ¢ deposition of a metal layer on a material (1 point) What occurs in electroplating? * ¢ aqueous hydrogen ion and hydroxyl ionġ9. (1 point) The products formed in the net reaction of the electrolysis of water are _. ¢ It uses an electric current to make a nonspontaneous reaction go.ġ8. ¢ It is the type of cell used in electrocution ¢ It changes chemical energy into electrical energy. (1 point) Which of the following is true about an electrolytic cell? * (1 point) When electrical energy is used to cause a chemical reaction we call this process _. ¢ hydrogen and oxygen are mixed before entering the anode.ġ6. ¢ hydrogen diffuses through the cathode. (1 point) In a hydrogen- oxygen fuel cell _. (1 point) To charge a lead storage battery you must _. (1 point) In the most common dry cell what material is the electrode that is the center rod made of? *ġ4. (1 point) What assures that there is no charge build up in a voltaic cell as oxidation and reduction occur? *ġ3. ¢ Either anode or cathode, depending on the metalġ2. (1 point) In a voltaic cell at which electrode does reduction occur? * ¢ Two half reactions must be physically separated.ġ1. ¢ One half reactions must involve more than one electron. ¢ Two half reactions must use a metal wire electrodes. ¢ One half reaction must involve two metals. (1 point) How must a redox reaction that is to be used as a source of electrical energy be set up? * (1 point) In a zinc-copper cell, Zn(s) | Zn^+2(1M) || Cu^+2(1M) | Cu(s), which electrode is positive? *ġ0. (1 point) Of the following metals, which ions are most easily reduced? Use the above table to answer the question. (1 point) Which atom has a change in oxidation number of +4 in the following redox reaction?K2Cr2O7 + H2O + S - > KOH + Cr2O3 + SO2 *Ĩ. (1 point) What is the oxidation number for each atom in NH4F? *ħ. (1 point) The oxidation number of oxygen when it is in a compound other than a peroxide is _. (1 point) What is the reducing agent in the following reaction? 2K + S - > K2S *ĥ. (1 point) Ag - > Ag ^+ +1 e^- This equation represents the type of reaction called _. ![]() (1 point) In the reaction of beryllium with fluorine, which atom is oxidized? *ģ. (1 point) What are transferred in an oxidation-reduction reaction? *Ģ. ![]()
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