193 Experiment 10: How to Make a Battery with Oxidation-Reduction 4. Part D of this experiment examines the effect of varying the concentrations of solutions in the anode and cathode compartments. Concentrations of 1.0 M, 1.0 x 10-2M, 1.0 x 10 M will be examined. While the 1.0 M concentrations are readily available, the other two concentrations should be prepared. For each of the desired solutions on the table below, calculate the amount of DI water to be added to the given stock solution. TABLE 10.1 DI Water to Add to Stock Solution (mL) Desired Solution Stock Solution 1.0 x 10-2 M Cuso, 1 mL of 1.0 M Cuse. 1.0 x 10 M CuSe. 1 mL of 1.0 × 10-M CYSQ. 1.0 x 102 M Znse. 1 mL of 1.0 M ZnSO, 1.0 x 10 M Znse. 1 mL of 1.0 × 10-2M ZnSQ. O. 5. Show the calculations for determining the volume of DI water to add to the given stock solution for the preparation of 1.0 x 102 M CuS0, and 1.0 x 10 M CUSO, solutions. Foc MacBo

193 Experiment 10: How to Make a Battery with Oxidation-Reduction 4. Part D of this experiment examines the effect of varying the concentrations of solutions in the anode and cathode compartments. Concentrations of 1.0 M, 1.0 x 10-2M, 1.0 x 10 M will be examined. While the 1.0 M concentrations are readily available, the other two concentrations should be prepared. For each of the desired solutions on the table below, calculate the amount of DI water to be added to the given stock solution. TABLE 10.1 DI Water to Add to Stock Solution (mL) Desired Solution Stock Solution 1.0 x 10-2 M Cuso, 1 mL of 1.0 M Cuse. 1.0 x 10 M CuSe. 1 mL of 1.0 × 10-M CYSQ. 1.0 x 102 M Znse. 1 mL of 1.0 M ZnSO, 1.0 x 10 M Znse. 1 mL of 1.0 × 10-2M ZnSQ. O. 5. Show the calculations for determining the volume of DI water to add to the given stock solution for the preparation of 1.0 x 102 M CuS0, and 1.0 x 10 M CUSO, solutions. Foc MacBo

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

Give a clear handwritten answer with explanation
Answer the following questions: Discuss the role of ion bridge or salt bridge in Electrochemical experiment. Explain thoroughly. How does a voltaic cell works in Electrochemical experiment? Explain thoroughly. What is a voltmeter in Electrochemical experiment? Explain thoroughly.
4. Sketch a Galvanic and an electrolytic cell, respectively for a redox reaction and label all the parts of the cell such electrodes, salt bridge and its salt, anode, cathode, voltmeter, salt solutions, flow of electrons, etc where and when applicable.
Can someone please help with question 10
Which statement is true a. Galvanic cells involve non-spontaneous redox reactions b. The oxidizing agents give off electrons C. In chemical cells the electrons flow from cathode to anode d. Electrolytic cells need an external source of electricity to proceed
Which of the following is the purpose of a salt bridge in an electrochemical cell? a. Stabilization of precipitates that may form during the redox reaction. b.Allowing the electrons to directly flow from anode to cathode. c. Providing electrons that react at the surface of the anode and cathode. d. Maintaining electrical neutrality by allowing ions to migrate.
6.
A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +Se Fe³+ (aq) +e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. half-reaction Write a balanced. equation for the Answer the following questions about this cell. 0 - Mn² (aq) + 4H₂O(1) Fe (aq) standard reduction potential +1.51 V Ered=+0.771 V 20 "red =
8. The electrolysis of copper (II) sulfate using carbon electrodes is demonstrated to a chemistry class. In the demonstration, a 1.50 A current passes through 75.0 mL of 0.125 mol/1. copper (II) sulfate solution. How long, in minutes, would it take to plate all of the copper from the solution?
If the given statement is true, write T. Otherwise, write F and explain why it is false 1)An electrolytic cell is used to generate electricity from chemical reactions 2) The reactant and the product need to have equal concentrations for a chemical reaction to be in equilibrium.
1) Construct a zinc-copper electrochemical cell using 1.0 M Zn2+ and 1.0 M Ni2+ solutions. a. Provide the shorthand notation. b. What is the EMF of this cell (include units)? c. For the voltage that you are measuring, is this E°cell or Ecell? Explain.
6. Copy the following diagram onto your answer sheet. Using the redox reaction given below, label the diagram with the following information: Beneath each beaker write the appropriate half reaction. Label each electrode with the appropriate metal. Indicate within each beaker the aqueous ion that is present inside the water. Along the wire indicate the flow of electrons using an arrow. On the salt bridge indicate which ion will flow into the anode and which ion will flow I. I. II. IV. V. into the cathode. Redox Reaction: Mg(s) + Sn²*(aq) → Mg²*(aq) + Sn(s) Salt Bridge: KNO3 salt bridge cathode anode