1. Explain the reasons of the color changes in litmus paper and in filter paper moistened withphenolphthalein 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 theredifferences between a storage battery and a Daniel cell?4. How many coulombs constitute 1 mole of electrons? Show your calculation.1065. 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 cellTake a glass tube bent twice at right angles and fill it with 3-5% NaCl solution. Plugthe open ends with cotton or glass wool. Connect this tube to the beakers as shown in Figure1. Make sure that there are no air bubbles inside the salt bridge. Place a clean copper strip inthe CUSO4 solution and a zinc strip in the ZnSO4 solution. Connect the two strips with a pieceof metallic wire and cut the wire in the middle. Place the cut ends of the wire in contact with aLitmus paper soaked in NaCl solution (The NaCl solution on the Litmus paper acts as anelectrolyte and will allow the flow of electrons from zinc to copper). Allow the current to flowfor a few minutes. Record any change of color of the Litmus paper. After a few minutes, theblue spot on the Litmus paper may become lighter in color. During this process keep theLitmus paper moistened with the NaCl solution and do not allow it to dry. Measure the cellpotential 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 moistenedwith NaCl and phenolphthalein solution instead of litmus paper.3. Measure the potential difference of the electrochemical cell consisting of 0.1M CUSO4 and0.01M ZNSO4 solutions as you did in step 1.4. Calculate the Gibbs free energy changes by using the potential differences measured insteps 1 and 3.5. Compare AG values and discuss the reasons.

The phenolphthalein indicator allows chemists to visually identify whether a substance is an acid or…

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

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

A common shorthand way to represent a voltaic cell is anode& anode solution& & cathode solution&cathode A double vertical line represents a salt bridge or a porous barrier. A single vertical line represents a change in phase, such as from solid to solution. Using the notation just described, represent a cell based on the following reaction: ClO3 -1aq2 + 3 Cu1s2 + 6 H+1aq2 ¡ Cl -1aq2 + 3 Cu2+1aq2 + 3 H2O1l2 Pt is used as an inert electrode in contact with the ClO3 - and Cl -. Calculate the standard cell emf given: ClO3 -1aq2 + 6 H+1aq2 + 6 e- ¡ Cl -1aq2 + 3 H2O1l2; E° = 1.45 V.
3. Consider the HCN-KCN buffer system, which species would react if a dilute aqueous HBr solution were added to the buffer? O CN O CN O HCN O KCN
How is the amount of current flowing through an electrolytic cell related to the amount of product produced in the redox reaction? Match the items in the left column to the appropriate blanks in the sentences on the right. multiplied coulombs Avogadro's 1 mol Faraday's 1g ampers 6.022 x 10¹ mol volts divided The number of moles of electrons that have flowed in a given electrolysis cell can be determined by measuring the total charge that has flowed through the cell. If the amount of current flowing through the cell is by the time that the current flowed, the total charge that passed through the cell in that time can be found. The relationship between charge and the number of moles of electrons constant, which corresponds to the charge in is given by of of electrons. These relationships are used to solve problems involving the stoichiometry of electrolytic cells. Reset Help
1. Draw a diagram that shows a battery made of three galvanic cells. How does the voltage of the battery compare with the voltage of its cells? | ©
5. Explain what is meant by a fuel cell. Provide a balanced equation to represent the reaction in any fuel cell of your choice.
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?
How do batteries generally work? If mercury batteries are so long lasting and efficient, then why are they not used anymore?
Select all that applyWhich of the following statements about galvanic cells are true? A. Reduction happens at the cathode and oxidation happens at the anode. B. The flow of electrons is from the cathode to the anode. C. The flow of electrons is from the anode to the cathode. D. Oxidation happens at the cathode and reduction happens at the anode.
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.
3.
Which of the following statements is(are) true for all galvanic cells? 1. Reduction occurs at the cathode. II. The anode gains mass during discharge (note: this means operation of the cell.) III. The voltage is less than or equal to zero. O only I O only III O only II O L I, and II O Il and II
What are the top 10 elements to build a battery out of? and why?