Homework Answers
Answer is option e, allows charge balance to be maintained in the cell.
In electrochemistry, the salt bridge is used to connect the oxidation and reduction half cells in a voltaic cell. It helps to maintain electrical neutrality within the cell and allows the ions to move from one half cell to another.
Without the salt bridge the negative and positive charges will build up around the electrodes causing the reactions to stop. Hence the function of salt bridge in a voltaic cell is to allows charge balance to be maintained in the cell.
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15. In voltaic cells, such as those diagrammed in your text, the salt bridge (a) is...
Question 16 (2 points) In voltaic cells, such as those diagrammed in your text, the salt...
Question 16 (2 points) In voltaic cells, such as those diagrammed in your text, the salt bridge O is not necessary in order for the cell to work. O acts as a mechanism to allow mechanical mixing of the solutions. O is tightly plugged with firm agar gel through which ions cannot pass. drives free electrons from one half-cell to the other. allows charge balance to be maintained in the cell. Pag Next Page Previous Page
Question 4 0.5 pts Which of the following statements about the salt bridge in a voltaic cell is false? The ions fro...
Question 4 0.5 pts Which of the following statements about the salt bridge in a voltaic cell is false? The ions from the salt bridge participate in the half-reactions, It allows electrical contact between the two solutions in the half-cells. It prevents mixing of the electrode solutions. It maintains the electrical neutrality in each half-cell .lons flow into and out of the salt bridge. Question 5 0.5 pts Which of the following statements about voltaic cells is false? Electrons flow...
12. All of the following statements concerning voltaic cells are true EXCEPT a) a salt bridge...
12. All of the following statements concerning voltaic cells are true EXCEPT a) a salt bridge allows cations and anions to move between the half-cells. b) electrons flow from the anode to the cathode in the external circuit. c) oxidation occurs at the cathode. d) a voltaic cell can be used as a source of energy, e) a voltaic cell consists of two-half cells. Answer:
What is the purpose of a "salt bridge" in a voltaic cell? a) It allows electrons...
What is the purpose of a "salt bridge" in a voltaic cell? a) It allows electrons to flow from the anode through the external circuit to the cathode. b) It is the electrode at which oxidation occurs. c) It is the electrode at which reduction occurs. d) It allows ions to migrate and maintain the electric neutrality in the half cells.
All of the following statements concerning voltaic cells are true EXCEPT O a voltaic cell consists...
All of the following statements concerning voltaic cells are true EXCEPT O a voltaic cell consists of two-half cells. electrons flow from the anode to the cathode. reduction occurs at the cathode. a salt bridge allows only cations to move between the half-cells. in the Zn2+/Zn-Cu/Cu2+ voltaic cell, Zn metal is the anode.
please and please choose the right answer and please make it clear for my understanding 1-Which...
please and please choose the right answer and please make it clear for my understanding 1-Which of the following statements are false? Oxidation and reduction half-reactions occur at electrodes in electrochemical cells All electrochemical reactions involve the transfer of electrons Oxidation occurs at the anode All voltaic (galvanic) cells involve the use of electricity to initiate nonspontaneous chemical reactions Reduction occurs at the cathode 2-During the electrolysis of aqueous KCl solution using inert electrodes, gaseous hydrogen is evolved at one...
question 16.46 UU 15 - UU UL ut tu uve- 16.46 The half-cells Fe2+ (aq)|Fe(s) and...
question 16.46
UU 15 - UU UL ut tu uve- 16.46 The half-cells Fe2+ (aq)|Fe(s) and O2(g)|H2O (in acid solution) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half- reactions and for the overall cell reaction. (b) Which half-reaction occurs in the anode compart- ment and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the — electrode to the electrode. Negative ions move...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
In this lab, we will explore how different voltaic cells work. 1. Prepare a voltaic cell...
In this lab, we will explore how different voltaic cells work. 1. Prepare a voltaic cell by placing the magnesium electrode and solution on the left, and the zinc electrode and solution on the right. Place the salt bridge between the two solutions. What is the voltage on this battery? 1.62v 2. Use the magnifying glass to look closely at the magnesium electrode and solution. a) What is happening at this electrode? Mg 2+ b) Write a half reaction showing...
1) High quality Au/Aus+ and Zn/Zn half-cells were connected with a salt bridge. Samples of water...
1) High quality Au/Aus+ and Zn/Zn half-cells were connected with a salt bridge. Samples of water containing traces of Au(III) ions were studied using Zn(s) dipped in 1.000 M Zn²+ and Au(s) dipped in the various water samples. Standard reduction potentials from your textbook are: Aut(aq) + 3e → Au(s) +1.42 V Zn²+ (aq) + 2e → Zn(s) -0.76 V a. Determine which half-reaction is the oxidation half-reaction and which is the reduction half-reaction. b. Determine the standard cell potential...
Question 16 (2 points) In voltaic cells, such as those diagrammed in your text, the salt bridge O is not necessary in order for the cell to work. O acts as a mechanism to allow mechanical mixing of the solutions. O is tightly plugged with firm agar gel through which ions cannot pass. drives free electrons from one half-cell to the other. allows charge balance to be maintained in the cell. Pag Next Page Previous Page
Question 4 0.5 pts Which of the following statements about the salt bridge in a voltaic cell is false? The ions from the salt bridge participate in the half-reactions, It allows electrical contact between the two solutions in the half-cells. It prevents mixing of the electrode solutions. It maintains the electrical neutrality in each half-cell .lons flow into and out of the salt bridge. Question 5 0.5 pts Which of the following statements about voltaic cells is false? Electrons flow...
12. All of the following statements concerning voltaic cells are true EXCEPT a) a salt bridge allows cations and anions to move between the half-cells. b) electrons flow from the anode to the cathode in the external circuit. c) oxidation occurs at the cathode. d) a voltaic cell can be used as a source of energy, e) a voltaic cell consists of two-half cells. Answer:
All of the following statements concerning voltaic cells are true EXCEPT O a voltaic cell consists of two-half cells. electrons flow from the anode to the cathode. reduction occurs at the cathode. a salt bridge allows only cations to move between the half-cells. in the Zn2+/Zn-Cu/Cu2+ voltaic cell, Zn metal is the anode.
question 16.46
UU 15 - UU UL ut tu uve- 16.46 The half-cells Fe2+ (aq)|Fe(s) and O2(g)|H2O (in acid solution) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half- reactions and for the overall cell reaction. (b) Which half-reaction occurs in the anode compart- ment and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the — electrode to the electrode. Negative ions move...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
In this lab, we will explore how different voltaic cells work. 1. Prepare a voltaic cell by placing the magnesium electrode and solution on the left, and the zinc electrode and solution on the right. Place the salt bridge between the two solutions. What is the voltage on this battery? 1.62v 2. Use the magnifying glass to look closely at the magnesium electrode and solution. a) What is happening at this electrode? Mg 2+ b) Write a half reaction showing...
1) High quality Au/Aus+ and Zn/Zn half-cells were connected with a salt bridge. Samples of water containing traces of Au(III) ions were studied using Zn(s) dipped in 1.000 M Zn²+ and Au(s) dipped in the various water samples. Standard reduction potentials from your textbook are: Aut(aq) + 3e → Au(s) +1.42 V Zn²+ (aq) + 2e → Zn(s) -0.76 V a. Determine which half-reaction is the oxidation half-reaction and which is the reduction half-reaction. b. Determine the standard cell potential...
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