Answered: Calculate Cell Potential (Ecell) of the…

Calculate Cell Potential (Ecell) of the following galvanic cell, (E° cell = 1.10 V) Zn(s) | Zn²+ (0.010 M) || Cu²+(1.0 M) | Cu(s) a. +1.10 V O b. -1.16 V O c. +1.16 V O d. -1.13 V O e. +1.13 V

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

Fe2+ (aq) + Zn(s) Fe(s) + Zn²+(09) E +0.32 V A galvanic cell generates a cell potential of +0.32 V when operated under standard conditions according to the reaction above. Which of the following pairs of conditions are needed to construct a similar cell that generates the lowest cell potential? A. [Zn2-] = 0.5 M and [Fe2+] =1 M because Q < 1 B. [Zn2-] = 1 M and [Fe2+] = 2 M because Q > 1 C. [Zn2-] = 2 M and [Fe2+] = 0.5 M because Q > 1 D. [Zn2-] = 2 M and [Fe2+] = 1 M because Q < 1
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
Calculate the cell potential of each of the following electrochemical cell at 25oC. a. Pt|H 2 (8.00 atm)|H + (1.00 x 10 -3 M)‖Ag + (0.00549 M)|Agb. Pt|H 2 (1.00 atm)| H + (pH = 5.97 ) ‖ H + (pH=3.47)|H 2 (1.00 atm)|Ptc. Pt|H 2 (0.0361 atm)|H + (0.0175 M)‖H + (0.0175 M)|H 2 (5.98 x 10 -4 atm)|Pt Please solve and give explanations steps.
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
e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
Referring to the table of Standard Cell Potentials below, determine the standard cell potential for the following reaction: Pb2+(aq) + 2 Cl-(aq) ---> Pb(s) + Cl2 E° Pb2+(aq) + 2e- ---> Pb(s) -0.126 Cl2 + 2e- ---> 2 Cl-(aq) +1.360
17. Calculate the cell potential of the cell described below: 2+ Al(s) | Al³+ (aq) (1.00 M) || Pb²+ (aq) (1.00 M) | Pb(s)
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5
10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V с. 0.60 V d. -0.60 V e. 0.095 V enstant fr ther
Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V
In the electrochemical cell shown here, the concentrations of Mn2+ and Cr3+ are 1.5x10-5 and 0.25 mol L-1, respectively. What is the cell potential? = E 0.0257 V -InQ KNO, Mn Mn(NO3)2 Cr(NO3)3 Mn* (aq) + 2e 2 Mn(s) E° =-1.18 V Cr* (aq) + 3e¯ 2 Cr(s) E° =-0.74 V