Abstract Chemical reactions can be used to produce electricity and electricity can be used to cause chemical reactions through oxidation-reduction reactions. The first part of the experiment measures the standard electrode potentials of five various half cells against the Cu2+(1M)|Cu half cell. The last three half cells are prepared through electrolysis. The electrode potentials of all reactions are positive which means that they are spontaneous. There is a significant percent difference from the
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Electrochemistry is a branch of chemistry that studies chemical reactions which take place in a solution at the interface of an electron conductor (a metal or a semiconductor) and an ionic conductor (the electrolyte)‚ and which involve electron transfer between the electrode and the electrolyte or species in solution. If a chemical reaction is driven by an external applied voltage‚ as in electrolysis‚ or if a voltage is created by a chemical reaction as in a battery‚ it is an electrochemical reaction
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using a glass hydronium ion selective electrode‚ a suitable reference electrode and a sensitive potentiometer (a pH meter) may be advantageous. THEORY Any acid-base titration may be conducted potentiometrically. Two electrodes‚ after calibration [to relate potential in millivolts (mV) to a pH value] are immersed in a solution of the analyte. One is an indicator electrode‚ selective for H3O+ and the other a stable reference electrode. The potential difference‚ which after calibration is
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toward Ni(s) (2) 2. Which processes occur during the electrolysis of molten sodium chloride? I. Sodium and chloride ions move through the electrolyte. II. Electrons move through the external circuit. III. Oxidation takes place at the positive electrode (anode). A. I and II only B. I and III only C. II and III only D. I‚ II and III (2) 3. What happens to the Cr3+(aq) ion when it is converted to CrO (aq)? A. Its oxidation number decreases and it undergoes reduction. B. Its oxidation number
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Chemistry 3202 Unit 4 Electrochemistry 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. Define the terms: oxidation and reduction in terms of loss or gain of electrons. P.714 Identify electron transfer in redox equations. P.714 Identify oxidation and reduction half-reaction equations in an oxidation-reduction (redox) equation. P.715- 716 Identify a redox equation as the sum of the oxidation half-reaction and the
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Experiment No. 3: Electrochemistry and Corrosion Date Performed: November 4‚ 2010 CONCLUSION Electrochemistry is a branch of chemistry that studies chemical reactions which take place in a solution at the interface of an electron conductor and an ionic conductor and which involve electron transfer between the electrode and the electrolyte or species in solution. Basically‚ an oxidation-reduction reaction (redox reaction) is a reaction in which electrons are transferred between species or in
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Isostatic Graphite: | | | | [pic] |[pic] | |Product Name：Isostatic Graphite | |
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41. In thylakoids‚ protons travel through ATP synthase from the stroma to the thylakoid space. Therefore the catalytic knobs of ATP synthase would be located a. on the side facing the thylakoid space b. on the ATP molecules themselves c. on the pigment molecules of PSI and PSII d. on the stroma side of the membrane e. built into the center of the thylkoid stack (granum) 42. Which of the following statements best represents the relationships between the light reactions and the Calvin cycle?
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half-cell is composed of an electrode (a strip of metal‚ M) within a solution containing Mn+ ions in which M is any arbitrary metal. The two half cells are linked together by a wire running from one electrode to the other. A salt bridge also connects to the half cells. Through electrochemistry‚ these reactions are reacting upon metal surfaces‚ or electrodes. An oxidation-reduction equilibrium is established between the metal and the substances in solution. When electrodes are immersed in a solution
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CHM 096 TUTORIAL 6 Mar 2013 (ELECTROCHEMISTRY) 1. Determine the oxidation number of the first name element in the following ions. a) Cr2O72 d) AsO33 b) SbF6 e) BaH2 c) MoO42 f) ClO4− 2. Determine whether each of the reactants shown in the following half-reactions is being oxidized or reduced. a) As4+ As3+ b) Cl2O7 HClO4 c) C2H4O C2H6O d) SO2 SO42− e) Cr2O72− Cr3+ 3. Indicate whether each of the following is or
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