9) Remove the metal wires from their solutions. Rinse them with water and dry them witha paper towel. Retain the copper wire and replace the zinc wire in the container in thehood.In-Lab Discussion1. When zinc metal reacts with Cu2+ ions, which substance is oxidized and which isreduced?2. Which metal is the anode in this electrochemical cell? Which is the cathode?3. In which direction do the electrons flow in this cell? From the zinc wire to thecopper metal wire, or vice versa?4. What would you conclude about the spontaneity of the reaction if you replaced the zincwire with another metal and found that the cell potential changed sign? Filter paperSaturated KNO; solution259Figure 1. Experimental apparatus.Experimental ProcedurePart 1. Copper and Zinc Metal1) Select a piece of copper and a piece of zinc metal wire from the containers in the hood.2) Clean the surface of the metal wires with the steel wool. Wipe clean with a dry papertowel.3) Obtain a plastic well plate. Fill one well with 10 drops of the Copper ion solution fromthe dropper bottle. Label this well with a Sharpie marker so that you remember whichsolution you filled it with,4) Repeat step 3 with Zinc ion solution. Select a well right next to the well in step 3 sothat the two wells with Copper and Zinc ion solution are right next to each other.5) Obtain a small dry strip of filter paper. You may have to cut a large piece of filterpaper down to the appropriate size. It should be exactly this big CIt's OK to tear the filter paper with your hands. Using the drop bottle, saturate the filterpaper strip with KNO; solution. Gently place one end of the filter paper into one of theion solution wells and the other end of the filter paper into the second ion solution well sothat a bridge is formed between the two solutions.6) Plug the alligator clips in to the voltmeter. The red lead connects to the voltmeter at theV Q Hz connection. The black lead connects to the COM connection. Connect the redalligator clip to one of the metal wires you chose and the black alligator clip to the othermetal wire you chose (make sure you clip on the metal and not the painted portion of thewire). Turn the voltmeter knob to 2 _V and power on by pressing .7) Dip both metal wires into their corresponding ion solutions and hold them there. If thereading from the voltmeter is negative, switch the alligator clips for the two metal wiresso that the potential is positive.8) Record the magnitude of the potential difference in the table provided.

Hello. There are multiple subparts in the question posted. The first three subparts have been…

9) Remove the metal wires from their solutions. Rinse them with water and dry them with a paper towel. Retain the copper wire and replace the zinc wire in the container in the hood. In-Lab Discussion 1. When zinc metal reacts with Cu2+ ions, which substance is oxidized and which is reduced? 2. Which metal is the anode in this electrochemical cell? Which is the cathode? 3. In which direction do the electrons flow in this cell? From the zinc wire to the copper metal wire, or vice versa? 4. What would you conclude about the spontaneity of the reaction if you replaced the zinc wire with another metal and found that the cell potential changed sign?

9) Remove the metal wires from their solutions. Rinse them with water and dry them with a paper towel. Retain the copper wire and replace the zinc wire in the container in the hood. In-Lab Discussion 1. When zinc metal reacts with Cu2+ ions, which substance is oxidized and which is reduced? 2. Which metal is the anode in this electrochemical cell? Which is the cathode? 3. In which direction do the electrons flow in this cell? From the zinc wire to the copper metal wire, or vice versa? 4. What would you conclude about the spontaneity of the reaction if you replaced the zinc wire with another metal and found that the cell potential changed sign?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

1. Consider the galvanic cell produced from the following unbalanced equation: Ce* + Mn*2 → Ce*3 + MnOs' a. Give the balanced net ionic equation for the reaction. b. Label the cell below with the electrodes, what is in each solution, and label the anode and cathode. Note the direction that electrons are moving in the sketch. Voltmeter Salt Bridge
QUESTION 39 Identify the location of oxidation in an electrochemical cell. O the salt bridge O the electrode O the socket the anode O the cathode
Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and F2(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. Fill 4 blanks ____
An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(??), dipping a cobalt rod in a solution of CoCl2(??), and connecting them with a wire and a salt bridge. In the cell that is constructed, the metallic zinc is being oxidized. a. Write cell line notation for the electrochemical cell. No include spectator ions. b. Doubling the mass of the zinc electrode from 5 g to 10 g will cause the measured voltage of the cell to, select one... (decrease, stay the same, increase,need more information) c. Increasing the concentration of zinc ions, Zn2+ , in solution will cause the measured voltage of the cell to, select one... (decrease, stay the same, increase,need more information)
5. Consider the following under acidic conditions: Cu(s) + MnO4¹-(aq) → Mn²+ + Cu²+ vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.
Place in a beaker of AgNO3 solution.2. Clean a piece of copper coin and a piece of silver coated coin.3. Connect the two coins to the opposite ends of a dry cell through a wire; the coppercoin to the negative end, and the silver coated coin to the positive end.4. Dip the 2 coins in the AgNO3 solution. What will happen? Explain in sentences
1. An electrochemical cell is made of two electrodes: (Zn²+/Zn) and (Ag+/Ag). Use the standard reduction potentials to answer the following questions. a. What is the standard potential of the cell and which electrode is the cathode and which one is the anode? b. Write a net redox equation for this electrochemical cell.
20
5. Consider a galvanic cell consisting of 5Fe?ag) + MnO1aq) + 8H°aq) → 5Fečaq) + Mnžia) + 4H201 Write the oxidation and reduction half-reactions and write the reaction using cell notation. Which reaction occurs at the anode? The cathode?
You have two beakers. One beaker contains 1 M Hg²* and 1 M Hg22*. The second beaker contains 1 M Fe2* and 1 M Fe*. All metals are present as their soluble nitrate salts. Design and draw a galvanic cell using these solutions (if you need other materials to complete the cell, you may add them in – state what they are needed for). Show the direction the electrons move (and where they move) and label the cathode and anode. Give the net ionic equation for the spontaneous reaction taking place in this galvanic cell. What would E°sell be?
I'm having some trouble on my homework and could really use some help See attached:
For a voltaic cell based on the reaction below, which statement is correct?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) a. Zn2+(aq) is oxidized at the anode. b. H+(aq) is reduced at the cathode. c. Zn2+(aq) is reduced at the anode. d. H2(g) is the oxidizing agent.