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2) Write half equations and net ionic equation for the above experiment. Calculate the cell potential using standard electrode potential table and compare it with the voltage obtained in the experiment. 3) For electricity to flow in a circuit, the circuit must be complete. What happens if you remove the salt bridge? Why?

2) Write half equations and net ionic equation for the above experiment. Calculate the cell potential using standard electrode potential table and compare it with the voltage obtained in the experiment. 3) For electricity to flow in a circuit, the circuit must be complete. What happens if you remove the salt bridge? Why?

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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Answers for Question 2 and 3 please.   

2) Write half equations and net ionic equation for the above experiment. Calculate the cell potential using standard electrode potential table and compare it with the voltage obtained in the experiment. 3) For electricity to flow in a circuit, the circuit must be complete. What happens if you remove the salt bridge? Why?
Transcribed Image Text:2) Write half equations and net ionic equation for the above experiment. Calculate the cell potential using standard electrode potential table and compare it with the voltage obtained in the experiment. 3) For electricity to flow in a circuit, the circuit must be complete. What happens if you remove the salt bridge? Why?
Anode → Zinc NO₂ Zn Zn Salt bridge Cu² K+ Cu²+ Cu (Zn² Zn(s)- Zn² (aq) + 2e- Cu(s) An electrochemical cell Results Measure the voltage produced by the cell. Record observations of the light globe, and any changes to the solutions and the electrodes. You should observe the cell working for a period of time. Discussion Questions 1) Explain what is happening in the above experiment (reduction/oxidation) in each part of the cell. [Where is oxidation occurring?, Where is reduction occurring?, which directions the ions and electrons are flowing] Electron flow Cathode O Copper Cu² Cu²+(aq) + 2e-
Transcribed Image Text:Anode → Zinc NO₂ Zn Zn Salt bridge Cu² K+ Cu²+ Cu (Zn² Zn(s)- Zn² (aq) + 2e- Cu(s) An electrochemical cell Results Measure the voltage produced by the cell. Record observations of the light globe, and any changes to the solutions and the electrodes. You should observe the cell working for a period of time. Discussion Questions 1) Explain what is happening in the above experiment (reduction/oxidation) in each part of the cell. [Where is oxidation occurring?, Where is reduction occurring?, which directions the ions and electrons are flowing] Electron flow Cathode O Copper Cu² Cu²+(aq) + 2e-
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