TUTOR Calculate the Concentration of a Species Using Cell Voltage When [Cu2+] = 1.39 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 1.196 V. What is the Zn2+ concentration in this cell? Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) [Zn2+] = mol/L
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- The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNiLearning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25∘C and standard conditions of 1 MM for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E∘−(2.303RT/nF) log10Q where E is the potential in volts, E∘ is the standard potential at 25 ∘C in volts, R=8.314J/(K⋅mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e−) is the Faraday constant, and Q is the reaction quotient. At the common reference temperture of 298 K, substituting each constant into the equation the result is E=E∘−(0.0592 V/n)log10Q a) Calculate the standard cell potential at 25 ∘C for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) b) What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 57 ∘C when [Fe2+]= 3.80 MM and [Mg2+]= 0.210 MM .When the Hg2+ concentration is 2.39×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.509V. What is the Zn2+ concentration? Hg2+(aq) + Zn(s) Hg(l) + Zn2+(aq)Answer: M
- Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀ Ti2+(aq)+Co(s) occurs at 25 °C, given that [Ti2 + ] = 0.00180 M and [Co2 + ] = 0.813 M. Refer to the table of standard reduction potentials. (Please give right answer)Show your work with tables 1 Amp means 1 C/1 sec 5 amp means 5C per 1 sec Faraday’s constant 96,485 C = 1 mole e- Write a balanced equations so you know mole ratio of e- to the solid you are electroplating Molar mass can be rounded to nearest 1/10th 89: How long will it take to plate out each of the following with a current of 100.0 A? 1.0 kG Al from aqueous Al3+ (book answer: 30 hours) 1.0 g Ni from aqueous Ni2+ (book answer: 33 s)When the Ag+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.658V. What is the Zn2+ concentration? 2Ag+(aq) + Zn(s)2Ag(s) + Zn2+(aq) Answer: M Submit Answer
- Answer all parts below, which are related to each other. The following electrochemical cell has a cell voltage of 0.033 V at 25 oC and 1.00 atmosphere pressure: Cu(s) | Cu2+(aq) (0.0010 M) || Cl-(aq) (0.10 M) | AgCl(s) | Ag(s) The following information is also known: Cu2+(aq) + 2e- <===> Cu(s) Eo = +0.339 V Ag+(aq) + e- <===> Ag(s) Eo = +0.7993 V A. Which electrode is the cathode, and why? Answer here: B. Find the [Ag+(aq)] in the right hand half-cell (compartment). Remember that AgCl(s) is very slightly soluble, so there will be some Ag+(aq) in the right side. While that is the end of this writing assignment, the answer key shows how to take things one step further and answer the more interesting chemical question of “What is the Ksp for AgCl(s)?”When the Pb2+ concentration is 5.46×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.147V. What is the Mg2+ concentration?Pb2+(aq) + Mg(s) Pb(s) + Mg2+(aq)Answer: MWhat is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 1.34 M and the Mg2+ concentration is 8.81×10-4 M ?Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)Answer: _____ VThe cell reaction as written above is spontaneous for the concentrations given: tue or false?
- What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 7.68×10-4 M and the Cr3+ concentration is 1.04 M ?3Pb2+(aq) + 2Cr(s)3Pb(s) + 2Cr3+(aq)Answer: _______ VThe cell reaction as written above is spontaneous for the concentrations given: (true/false)When the Cu2+ concentration is 3.82×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.893V. What is the Al3+ concentration?3Cu2+(aq) + 2Al(s)----> 3Cu(s) + 2Al3+(aq)Answer: ____ MWhen the Ag+ concentration is 1.07 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.665V. What is the Zn2+ concentration? 2Ag+(aq) + Zn(s) → 2Ag(s) + Zn2+(aq) Answer:_____ M