Q: Sketch a diagram of the galvanic cells
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Q: Describe the process of calculating Concentrations in a Voltaic Cell?
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Q: Question attached
A: Hello. Since the question contains multiple subparts, the first three subparts are solved. In case…
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Q: What is electrochemical cell?
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A: Redox reaction are those in which both oxidation and reduction reaction takes place simultaneously.
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A: We'll answer the first question since the exact one wasn't specified. Please submit question…
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Q: What are the main components of an electrochemical cell?
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A: ANSWER IS DISCUSSED BELOW :
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Q: what electrochemical reaction uses in silver oxide battery
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Q: Give two examples of an electrochemical cell.
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A: Electrochemical cell:
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Q: What is overvoltage in an electrochemical cell? Why is it important?
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- Give Reason? (i) Why is a high supporting electrolyte concentration used in most electroanalyticalprocedures?(ii) Why is the reference electrode placed near the working electrode in a threeelectrode cell?Give the calomel electrode half cell diagram. What equailibria control the electrod potential of calomel electrode?In the analysis at 25 ° C of chloride using an ion selective electrode (ISE), two 100 mL solutions were prepared. These contain 1.0129x10-2 M and 1.01239x10-3 M Cl- and yielded a potential of 20.3 mV and 79.5 mV, respectively. The value of the electrode slope in mV is:
- What is the difference between an active and an inactiveelectrode? Why are inactive electrodes used? Name two sub-stances commonly used for inactive electrodes.The main advantage of using a saturated KCl solution at the reference electrode is,A. Potassium chloride is cheapB. Easy reaction with analyteC. Easy passage of chloride ions through membranesD. The chloride concentration does not change when the liquid evaporates from the cellUse the shorthand notation to describe a cell consisting of a saturated calomel reference electrode and a silver indicator electrode for the measurement of (a) pSCN. (b) pI. (c) pSO3 (d) pPO. Then, generate an equation that relates pAnion to Ecell for each of the cells. (For Ag2SO3 Ksp = 1.5 * 10-14; for Ag3PO4, K,p = 1.3 *10-20 ).
- Given the following: A cell SCE // Ag2CrO4 (saturated), CrO42- (xM) /AG is used for the determination of pCrO4- (ESCE = -0.244 V at 25 C). The half reaction at indicator electrode is: Ag2CrO4(s) + 2e- 2 Ag(s) + CrO42- (E0 = +0.446 V) What is pCrO4, given the cell potential of 0.402? What type of indicator electrode is Ag in this situation?What Range of cathode potentials versus the saturated calomel electrode can be used to quantitatively separate Ag+ and Ni2+ by electrolytic deposition? Assume that the sample solution is initially 0.1000M in each ion and the quantitative removal of an ion is realized when only 1 part in 10000 remains undeposited. ESCE = 0.244V E0Red (Ag+) = 0.8V E0Oxid (Ni) = -0.25VWhich property is not desirable in an ideal reference electrode? a. Reproducibility b. First kind electrode c. Thermal stablity d. Reversible electrode
- What is the aim of submerging the electrode in a potassium chloride solution? Must this be stored in a distilled or deionized water? What is the aim of measuring the pH meter utilizing reference buffers?Why is SHE considered as the standard electrode?The Zn-Cl battery has been suggested as an energy generator in transportation. The reactionis as follows:Zn (s) + Cl2 (g, 1 atm.) ZnCl2 (aq)a) It the molality of the electrolyte ZnCl2 is of 0.1 m, employ the Debye-Hückel law for calculating the average ionic activity coefficient (γ±), the average ionic activity (a±) and theelectrolyte’s activity (a2) b) Calculate the cell potential (Ecell), at 25 °C, using the values obtained in the previous section. Result a) γ±= 0.2768; a±=0.0440; a2=8.512 10-5 b) 2.2434 V