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1. Explain the reasons of the color changes in litmus paper and in filter paper moistened witl phenolphthalein solution. 2. Write balanced equations for all reactions taking place in the system. 3. Do you know how a storage battery (car battery) works? What are the reactions? Are there differences between a storage battery and a Daniel cell? 4. How many coulombs constitute 1 mole of electrons? Show your calculation.

1. Explain the reasons of the color changes in litmus paper and in filter paper moistened witl phenolphthalein solution. 2. Write balanced equations for all reactions taking place in the system. 3. Do you know how a storage battery (car battery) works? What are the reactions? Are there differences between a storage battery and a Daniel cell? 4. How many coulombs constitute 1 mole of electrons? Show your calculation.

Chemistry
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...
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1. Explain the reasons of the color changes in litmus paper and in filter paper moistened with phenolphthalein solution. 2. Write balanced equations for all reactions taking place in the system. 3. Do you know how a storage battery (car battery) works? What are the reactions? Are there differences between a storage battery and a Daniel cell? 4. How many coulombs constitute 1 mole of electrons? Show your calculation. 106 5. What are the meanings of positive and negative reduction potentials?
Transcribed Image Text:1. Explain the reasons of the color changes in litmus paper and in filter paper moistened with phenolphthalein solution. 2. Write balanced equations for all reactions taking place in the system. 3. Do you know how a storage battery (car battery) works? What are the reactions? Are there differences between a storage battery and a Daniel cell? 4. How many coulombs constitute 1 mole of electrons? Show your calculation. 106 5. What are the meanings of positive and negative reduction potentials?
Procedure: 1. Take two 50 mL beakers. In one beaker, add 30 mL of 0.1M CUSO4 solution and in another, 30 mL of 0.1M ZNSO4 solution. The preparation of salt bridge and set-up of the cell Take a glass tube bent twice at right angles and fill it with 3-5% NaCl solution. Plug the open ends with cotton or glass wool. Connect this tube to the beakers as shown in Figure 1. Make sure that there are no air bubbles inside the salt bridge. Place a clean copper strip in the CUSO4 solution and a zinc strip in the ZnSO4 solution. Connect the two strips with a piece of metallic wire and cut the wire in the middle. Place the cut ends of the wire in contact with a Litmus paper soaked in NaCl solution (The NaCl solution on the Litmus paper acts as an electrolyte and will allow the flow of electrons from zinc to copper). Allow the current to flow for a few minutes. Record any change of color of the Litmus paper. After a few minutes, the blue spot on the Litmus paper may become lighter in color. During this process keep the Litmus paper moistened with the NaCl solution and do not allow it to dry. Measure the cell potential by a voltmeter. Record the observations and explain the reasons. 2. Repeat the same experiment carried out in step 1 using a piece of filter paper moistened with NaCl and phenolphthalein solution instead of litmus paper. 3. Measure the potential difference of the electrochemical cell consisting of 0.1M CUSO4 and 0.01M ZNSO4 solutions as you did in step 1. 4. Calculate the Gibbs free energy changes by using the potential differences measured in steps 1 and 3. 5. Compare AG values and discuss the reasons.
Transcribed Image Text:Procedure: 1. Take two 50 mL beakers. In one beaker, add 30 mL of 0.1M CUSO4 solution and in another, 30 mL of 0.1M ZNSO4 solution. The preparation of salt bridge and set-up of the cell Take a glass tube bent twice at right angles and fill it with 3-5% NaCl solution. Plug the open ends with cotton or glass wool. Connect this tube to the beakers as shown in Figure 1. Make sure that there are no air bubbles inside the salt bridge. Place a clean copper strip in the CUSO4 solution and a zinc strip in the ZnSO4 solution. Connect the two strips with a piece of metallic wire and cut the wire in the middle. Place the cut ends of the wire in contact with a Litmus paper soaked in NaCl solution (The NaCl solution on the Litmus paper acts as an electrolyte and will allow the flow of electrons from zinc to copper). Allow the current to flow for a few minutes. Record any change of color of the Litmus paper. After a few minutes, the blue spot on the Litmus paper may become lighter in color. During this process keep the Litmus paper moistened with the NaCl solution and do not allow it to dry. Measure the cell potential by a voltmeter. Record the observations and explain the reasons. 2. Repeat the same experiment carried out in step 1 using a piece of filter paper moistened with NaCl and phenolphthalein solution instead of litmus paper. 3. Measure the potential difference of the electrochemical cell consisting of 0.1M CUSO4 and 0.01M ZNSO4 solutions as you did in step 1. 4. Calculate the Gibbs free energy changes by using the potential differences measured in steps 1 and 3. 5. Compare AG values and discuss the reasons.
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