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?

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?

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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Substances A2, B2, and C2 can all act as oxidizing agents. In solution, A2 is green, B2 is yellow, and C2 is red. In the reactions in which they participate, they are reduced to A, B, and C ions, all of which are colorless. When a solution of C2 is mixed with one containing B ions, the color changes from red to yellow. Which species is oxidized? __________ Which is reduced? __________ When a solution of C2 is mixed with one containing A ions, the color remains red. Is C2 a better oxidizing agent than A2? __________ Is C2 a better oxidizing agent than B2? __________ Arrange A2, B2, and C2 in order of increasing strength as an oxidizing agent. ___________________ _______________ ______________ weakest oxidizing agentstrongest oxidizing agent
From the experiment below, what are your observation? Please provide 3-5 sentences of your observation in your own words.Also, question number 1:In the apple oxidation experiment, which apple slice did you think was oxidized first? Why is that so?
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
In the electrochemical system, what is being described by the following? positive electrode negative electrode require electricity in order for redox to take place produces electricity during redox reaction electrode where reduction would usually take place Spontaneous reaction will occur A. galvanic cell B. electrolytic cell C. Cathode D. anode
1. Which of the following statements is / are TRUE for ELECTROCHEMISTRY? A. The electricity from a battery can be used to transfer the electrons of an atom to another. B. It results from the movement of atoms between one atom to another. C. It is the relationship between chemistry and electricity. D. It involves the movement of electrons due to RedOx reactions. E. Chemical reactions cannot make electricity flow. F. Electricity makes some chemical reactions possible 2. Which of the following statements is / are TRUE for a GALVANIC CELL? A. It is also known as voltaic cell. B. It is the device used to generate electricity from chemical reactions.
The diagram shows electroplating of a steel object. A student made the statements 1 to 3 in the picture below. Which statements are correct? steel object copper- copper(ll) sultate solution A student made the following statements. 1 The object turns a reddish-brown colour. 2 The copper sulfate solution changes to a paler blue colour. 3. The copper electrode becomes smaller.
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 each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. Write the chemical formulae of any reactants that will be reduced in the third column. reaction JC1, () +2A1() SC(s) +S() 1₂(0)+ Ma(0) ZAICI, () Cas() Mal₂ (0) reactants oxidized 0 0 0 reactants reduced 0 0 0 X
Redox reactions occur in many everyday experiences. Three examples of common redox reactions that everyone is familiar with are outlined below. Write the chemical equation for each of these reactions and identify the oxidizing agent and the reducing agent. Note: If needed, consult a web source to determine the reaction. a. When silver jewelry or silverware tarnishes, it is reacting with S in the air to undergo a redox reaction. b. When someone leaves a screwdriver sitting outside and it rusts, the iron in the screwdriver underwent a redox reaction. c. The process of photosynthesis, which causes green plants to react with sunlight to form oxygen, is an example of a redox reaction.
The idea behind this problem is to balance the redox reaction on a separate piece of paper until you are finished. Then place the correct coefficients in front of each of the species in the balanced reaction. Before each chemical species is a box in which you are to type the number of the coefficient. Where there is a blank, there are two boxes. The box before the blank is for the coefficient. Type the number into this box. The box after the blank is asking the formula of the compound that goes there. This formula will be either H+, OH-, or H2O. Please type them in this way. When the following redox reaction is balanced in BASIC solution (blanks indicate either H*, OH", or H20) MnO2(s) + CIO"(aq) + MnO4 (aq) + CI (aq) + - The correct coefficients in front of each species are (Left side of the arrow) MnO2(s) CIO (aq) Enter coefficient here Enter H+, OH-, or H2O here (Right side of the arrow) MnO4-(aq) cr(aq) Enter coefficient here Enter H+, OH-, or H2O here
A steel bumper is placed in an electroplating cell as the cathode. An electric current of 5.77 A flows through the cell for 30.0 minutes. The cell contains a solution of 2.00 mol/L solution of chromium (III) nitrate. 10. Determine the mass of chromium that will be plated onto the bumper in 30.0 minutes?
Why must electrolysis reactions occur at the electrodes in order for electrolytic conduction to continue? Select the single best answer. a. Otherwise the electrodes would run out of electrons and the system would cease to function. b. Otherwise the electrodes would accumulate charge and the system would cease to function. c. Otherwise the electrodes would become inert and the system would cease to function. d. Otherwise the electrodes would not accumulate charge and the system would cease to function.