QUESTION 31Caiculate the cell potential, Ecell, for the following voltaic cell, given IN2+ = 0.07 M and [Zn2+j = 0 85 MZn(s) + Ni2*(aq) - Ni(s) + Zn? (ag)O +0.50 VE= 0 53 VO +0 48 VO +0 57 VO +0.59 VO +0.55 VQUESTION 32How many electons does each oxygen atom loselgain in the redox reaction below?4 Al(s) + 3 O2(g)2 Al208($)O each oxygen loses 1 électrofO each oxygen gains 1 electronO each oxygen loses 2 électronsO each oxygen gains 2 electronsO each oxygen loses 4 electronsO each oxygen gains 4 electrons

31. Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Calculate the cell potential, Ecell, for the following voltaic cell, given (N2+=0.07 M and (Zn2+) = Zn(s) + Ni2*(aq)- Ni(s) + Zn? (aq) O +0.50 V 330 85 M E=053 V +0 48 V O +0 57 V +0.59 V O +0.55 V QUESTION 32 How many electons does each oxygen atom lose/gain in the redox reaction below? 4 Al(s) + 3 02(g)2Abos) O each oxygen loses 1 blectron O each oxygen dains 1 electron O each oxygen loses 2 électrons each oxygen gains 2 electrons O each oxygen loses 4 electrons each oxygen gains 4 electrons

Calculate the cell potential, Ecell, for the following voltaic cell, given (N2+=0.07 M and (Zn2+) = Zn(s) + Ni2*(aq)- Ni(s) + Zn? (aq) O +0.50 V 330 85 M E=053 V +0 48 V O +0 57 V +0.59 V O +0.55 V QUESTION 32 How many electons does each oxygen atom lose/gain in the redox reaction below? 4 Al(s) + 3 02(g)2Abos) O each oxygen loses 1 blectron O each oxygen dains 1 electron O each oxygen loses 2 électrons each oxygen gains 2 electrons O each oxygen loses 4 electrons each oxygen gains 4 electrons

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 69E: Consider the concentration cell shown below. Calculate the cell potential at 25C when the...

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The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
You have a concentration cell with Cu electrodes and [Cu2+] = 1.00 M (right side) and 1.0 104M (left side). a. Calculate the potential for this cell at 25C. b. The Cu2+ ion reacts with NH3 to form Cu(NH3)2+ by the following equation: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 Calculate the new cell potential after enough NH3 is added to the left cell compartment such that at equilibrium [NH3] = 2.0 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)
Part B: The Nernst EquationWrite the Nernst equation2 for the reaction Cu2+ (aq) + Zn (s)  Zn2+ (aq) + Cu (s)Let activity of Cu2+ equal to 1 and change the activity of Zn2+ such that Q is in the range  0.001 to +0.001. Select different values of Q and for each calculate Ecell. Plot E_"cell" -E_"cell" ^ө vs ln Q. What is the effect of Q (that is the activity) on E_"cell" -E_"cell" ^ө ? Is the effect the same at higher and lower values of Q? what is the largest value of the absolute difference between cell potential and standard cell potential, |E_"cell" -E_"cell" ^ө |? What do you expect the graph will look like for different number of electron transferred ( )? And why?
show full solution A galvanic cell is constructed from a silver half-cell and a copper half-cell. The copper half-cell contains 0.10M Cu(NO3)2 and the concentration of silver ions in the other half-cell is unknown. If the silver electrode is the cathode and the cell emf is measured and found to be 0.10 v at 25oC, what is the Ag+ ion concentration?
Given the following cells in one container: Pt(s) | Cu^+ (aq), Cu^2+ (aq) | | Cu^+ (aq) | Cu(s), where E° red Cu^+/Cu^+ = 0.15 V and E° red Cu^+/Cu = 0.52 V. Calculate the Ecell given [Cu^+] = 0.53 M and [Cu2^+] = 0.27 M and calculate the △G for the cell
INTERACTIVE EXAMPLE Electroplating How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 108.4 A? HOW DO WE GET THERE? Question Content Area How long will it take to plate out 3.0 g Ni with the 108.4 A current? ________s
A voltaic cell is constructed with two Fe2+-Fe electrodes, where the half-reaction is Fe2+(aq)+ 2e – → Fe(s) E° = –0.45 V The concentrations of Fe2+ ion in the two compartments are 0.0088 M and 1.23 M. What is the cell potential at 298 K? Express your answer to two significant figures. Ecell = Answer V
3. How long will it take to electrodeposit 1.05 g Cr from 0.504 M Cr2O72- solution if 3.10 A current ispassed through the solution?A. 15082 s B. 1257 s C. 7541 s D. 2338 s E. 3770 s
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Learning 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 .