Write out what data and information you plan to collect during the experiment of electrochemistry redox reaction (Oxidation Reduction) to answer how will a species be reduced or gain electrons when a species is oxidized??Then list the equations and formulas you plan to use to manipulate that data.Also list how many trials you plan to do?

Write out what data and information you plan to collect during the experiment of electrochemistry redox reaction (Oxidation Reduction) to answer how will a species be reduced or gain electrons when a species is oxidized??Then list the equations and formulas you plan to use to manipulate that data.Also list how many trials you plan to do?

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter19: Redox Reactions

Section: Chapter Questions

Problem 89A

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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.…
For an electrolytic cell experiment, which will contribute to the greatest source of error on the mass of the deposited metal? Select one: A. The experiment was done at a higher temperature. B. A higher voltage was applied in the electrolyte solution. C. The electrolyte solution was accidentally diluted with water. D. The electrodes were weighed immediately after removing them from the solution.
Why did Volta doubt results from Galvani's first round of animal electricity experiments? A. He believed in the droplet theory of nerve function and thought muscle contraction was dependent on metal and liquid interaction. B. He determined that only copper was critical for muscle contraction C. He has evidence that simply having two different metals near a nerve could produce similar results D. He could in no way replicate Galvani's experiments
For an electrolytic cell experiment, which will contribute to the greatest source of error on the mass of the deposited metal? Select one: A. The experiment was done at a lower temperature. B. The electrolyte solution was more concentrated than the reported concentration. C. A lower voltage was applied in the electrolyte solution. D. The electrodes were not pre-weighed and were weighed after the deposited metal was removed.
1. Introduction to Electrochemistry a. What are the two ways where chemical reactions and electricity interact? b. In the Galvanic cell, has a weaker pull for electrons and has a strong pull for electrons. c. What information can be derived from the table of Standard Reduction Potentials? d. In the Galvanic cell, the piece of zinc is the (it is where oxidation happens).
What do you think you will be doing in the electrochemistry redox reaction (Oxidation Reduction) experiment, and then answer- Will a species be reduced or gain electrons when a species is oxidized? Also, you should explain how you plan to use the different chemicals, glassware, tools, and equipment?
None
A pathway by which counter ions can flow between the half-cells of a galvanic cell without the solutions in the half-cell totally mixing is provided by A. the anode B. the cathode C. the electrode D. the salt bridge E. the wire connecting the half-cells
The redox reaction happening in a galvanic cell permits the flow of what kindof particle shown in a voltmeter? A. Electrolyte B. Electrons C. Neutrons D. Protons
d. Provide the overall balanced equation for this galvanic cell. e. Write the line notation for the cell. f. Calculate the standard cell potential.
In this section, you should record any visual observations you make (colors, appearances of water, physical states, etc) for electrochemistry redox reaction (Oxidation Reduction)experiment. You should also record any numeric observations (masses, volumes, concentrations).Make sure they are organized and labeled so it is clear what the observation of electrochemistry redox reaction (Oxidation Reduction)experiment. Here is the data for the electrochemistry redox reaction (Oxidation Reduction)experiment: The first part was testing the observed vs theoretical cell potentials for the following voltaic cells: Zn/Cu reading was 0.914 Zn/Al reading was 0.210 Zn/Ag reading was 1.330 Al/Cu reading was 0.672 Ag/Cu reading was 0.413 Ag/Al reading was 1.000 The second part of the experiment was constructed an electrolytic cell using 2.008 grams of KI in about 100mL of DI water. Then measured the pH of the reaction mixture which was 5.22 with soultion in plain water and 10.74 with soultion added.
In this section, you should record any visual observations you make (colors, appearances of water, physical states, etc) for electrochemistry redox reaction (Oxidation Reduction)experiment. You should also record any numeric observations (masses, volumes, concentrations).Make sure they are organized and labeled so it is clear what the observation of electrochemistry redox reaction (Oxidation Reduction)experiment. Here is the data for the electrochemistry redox reaction (Oxidation Reduction)experiment: Part 1 was testing the observed vs theoretical cell potentials for the following voltaic cells: Zn/Cu reading was 0.914 Zn/Al reading was 0.210 Zn/Ag reading was 1.330 Al/Cu reading was 0.672 Ag/Cu reading was 0.413 Ag/Al reading was 1.000 Part 2 of the experiment was constructed an electrolytic cell using 2.008 grams of KI in about 100mL of DI water. Then measured the pH of the reaction mixture which was 5.22 with soultion in plain water and 10.74 with soultion added.