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- 1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3¯ into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. b. Write the balanced (ionic) redox equation for the conversion of Br into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of Ht: HBr and CH3COOH)1. The formation of molecular bromine (Br2) from HBr and KBгO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br₂ under acidic conditions. Label the half reaction as either oxidation or reduction. b. Write the balanced (ionic) redox equation for the conversion of Br into Br₂ under acidic conditions. Label the half reaction as either oxidation or reduction. C. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of H+: HBr and CH3COOH) 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations. (Note that…Which change in oxidation number represents reduction? Choose the right answer in the given choices below: a.) –1 to +1 b.) –1 to –2 c.) –1 to 0 d.) –1 to +2
- What reaction is involved? reduction or oxidation?Identify the statements whether true or false. Select T if true, and F if false. a. Redox reactions occur by the movement of electrons. b. Galvanic cells generate electricity by a spontaneous redox reaction. c. In electrolytic cells, non-spontaneous reaction is made spontaneous by means of electricity. d. Electrons are consumed at the positive terminal (electrode). e. Cations are attracted to the anode in electrolytic cells. f. The metal that is to be electroplated is attached to the anode. g. The anode has the more positive Eo half-cell. h. The more positive the Eo cell, the stronger oxidizing agent. i. The standard reduction potentials are measured at 25oC. j. The oxidation number increase at the cathode.2. a gain in oxygen during this process is called reduction process A. True B.False
- Consider the equation on the picture. A.What is the balance oxidation reaction? B.What is the balance reduction reaction.1. Balance the following equation using the half-reaction method discussed in experiments 7 and 8. Pay careful attention the condition of the reaction. b. Which element is reduced? SHOW the change in electrons. [ɔisval ON +(HO)nɔ + _ON +nɔ Which element is oxidized? SHOW the change in electrons.Worksheets! WORKSHEET 2 Part I. Read and answer the following questions. 1. What is oxidation? 2. What is reduction? 3. Electron-accepting species which tend to undergo a reduction in redox reactions are called 4. Write the 4 conventional kinds of primary batteries. 5. Explain the hazards of using batteries. 6. List at least 3 examples of objects that are powered by primary batteries. C. a. b. 7. List at least 3 examples of objects that are powered by secondary batteries. 8. For electrochemical corrosion to occur, three ingredients must be present. Those are: b. a. C. 9. TRUE or FALSE. During electrolysis, ionic substances are decomposed into simpler. substances when an electric current is passed through them. 10. TRUE or FALSE. One of the factors affecting electrolysis is the undervoltage of the electrodes. Part II. Choose the letter of the best answer. 1. It can be defined as a chemical reaction in which electrons are transferred between two reactants participating in it. a.…
- Tarnished silver can be restored by contact with magnesium in a salt solution. In this reaction, the tarnished silver is reduced. What is oxidized?EQUATIONS 1. The formation of molecular bromine (Br2) from HBr and KBrO3 must be derived using redox reactions. a. Write the balanced (ionic) redox equation for the conversion of BrO3 into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. b. Write the balanced (ionic) redox equation for the conversion of Br¯ into Br2 under acidic conditions. Label the half reaction as either oxidation or reduction. c. Write the balanced net (ionic) redox reaction (reduced to the lowest whole number coefficients) d. Rewrite the balanced net redox equation in complete (molecular) form using KBrO3, HBr and CH3COOH as the reactants. (note that this step may require a bit of manipulation as there are two sources of Ht: HBr and CH3COOH) 2. Write the equation for the reaction of acetanilide with molecular bromine (for the organic compounds, draw the full structures, not condensed formulae). 3. Write the balanced equation for this experiment by adding these two equations.…Part a) Identify the oxidation numbers for all the species. Part b) Look at the oxidation numbers and determine what reactant is the one being reduced and which one is being oxidized? Part c) Explain how you determined your choices in Part b.
