A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a solution of ZnSO4. The Zn wire is attached to the positive terminal and the Ag/AgCl electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn²+] in the solution if the cell potential, E cell, is -1.098 V. The standard reduction potential of the Zn² +/Zn half- reaction is -0.762 V. [Zn²+] = M

A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a solution of ZnSO4. The Zn wire is attached to the positive terminal and the Ag/AgCl electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn²+] in the solution if the cell potential, E cell, is -1.098 V. The standard reduction potential of the Zn² +/Zn half- reaction is -0.762 V. [Zn²+] = M

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...

See similar textbooks

Similar questions

consider these two entries from a ficitional table of standard reduction potentials. (see image) what is the standard potential of a galvanic (voltaic) cell? give answer to 3 sig figs inputting only the numeric value, assuming a measurement of V
The potential of the following cell was measured as 182 mV. (oEAg+/Ag=0.8 V) Ag (s)| Ag+ (0.01M) || VO2+ (0.1M), VO2+ (0.1M), H+ (0,1 M)| Pt (s) Drive a figure for this cell and write the anodic and cathodic reactions. Calculate the standard redox potential of the VO2+/VO2+
One-half of an electrochemical cell consists of a pure nickel electrode in a solution of Ni2+ ions; the other half is a cadmium electrode immersed in a Cd2+ solution. Use the following standard emf series Table (if required). Standard Electrode Electrode Reaction Potential, V" (V) Au³+ + 3e → Au +1.420 O2 + 4H+ + 4e Pr2+ + 2e 2H2O +1.229 Pt -+1.2 Ag+ + e Fe+ + e → Ag Fe2+ +0.800 +0.771 Increasingly inert (cathodic) O2 + 2H,O + 4e Cu²+ + 2e 4(OH) +0.401 Cu +0.340 2H* + 2e Pb2+ + 2e H2 0.000 Pb -0.126 Sn2+ + 2e Sn -0.136 Ni2+ + 2e Ni -0.250 Co2+ + 2e Cd²+ + 2e Fe+ + 2e Co -0.277 Cd -0.403 Fe -0.440 Cr+ + 3e Cr -0.744 Increasingly active (anodic) Zn2+ + 2e¯ Zn -0.763 AF+ + 3e Al -1.662 Mg²+ + 2e Mg -2.363 Na+ + e –→ Na -2.714 K* + e -→ K -2.924 If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V Ni + Cd2+ ---> Ni2+ + Cd and +0.153 V Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V Ni + Cd2+ Ni2+ + Cd…
A voltaic cell employs the redox reaction:Ba(s) + 2 Ce4+(aq) → 2 Ce3+(aq) + Ba2+(aq) E°cell = 4.51 VCalculate the cell potential 25 °C when [Ce4+] = 5.54×10-4 M and [Ce3+] = [Ba2+] = 3.58 M. 4.38 V 4.27 V 4.75 V 4.03 V 4.64 V
The Na + concentration of a solution was determined by measurements performed with a sodium ion selective electrode. The electrode system has developed a potential for - 0.2831 V when immersed in 15.00 mL of the solution of unknown concentration. After adding 5.00 mL of NaCℓ 1.00 x 10-2 mol / L to the solution of unknown concentration, the potential went to -0.1546 V. Calculate the Na + concentration in the original solution.
Determine the potential of cell under with the measured conditions Er(s)|Er2+(aq)||Qi+(aq)| Qi(s) Concentration of Er2+ is 1.5 Concetration of Qi+ is 1.89 E cell of half reaction of Er2+ = .963 E cell of half reaction of Qi = 1.305
Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
Calculate the theoretical potential of the following cell and indicate whether the reaction will proceed spontaneously in the direction considered Zn Zn²+ (0.0350 M) | Ti³+ (9.06 x10-² M), Tit (0.0200 M)| Pt
is 0.085 correct or should it be 0.116? I got two answers and i’m not sure.
Calculate the theoretical cell potential of the following cells. If the cell is short-circuited, indicate the direction of the spontaneous cell reaction. Zn/Zn²+ (0.1000 M) // Co²+(5.87 x 104 M)/ Co Ez2+ = -0.763V E Co2+ = -0.277V O +0.419 V spontaneous reaction +0.422 V spontaneous reaction O +0.421 V spontaneous reaction +0.420 V spontaneous reaction
50.0 mL of 0.100 M Co3+ solution is titrated with 35.00 mL of 0.130 M MnO42- solution. The potential is measured against the Ag-AgCl reference electrode. Find the measured cell potential. E0 (Ag/AgCl) = 0,197 V Co3+ + e- ↔ Co2+ E0 = 1,92 V MnO4- + e- ↔ MnO42- E0 = 0,56 V