Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e - Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 V

Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e - Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 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

If the following half-cells are the right-hand electrode in a galvanic cell with a standard hydrogen electrode on the left, calculate the cell potential. If the cell were shorted, indicate whether the electrodes shown would act as an anode or a cathode. a) Ag |AgI(sat’d), KI(0.0898 M) b) Pt |Sn2+(0.0893 M), Sn4+(0.215 M) c) Ag|Ag(S2O3)2 3- (0.00891 M), Na2S2O3(0.1035 M)Required to answer. Single line text.
What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 45°C and the operating pressure is 0.06 atm. Fe2+(aq) + 2 e− ↔ Fe(s) ; [Fe2+] = 2.25 M E0 = −0.44 V Ag+(aq) + e− ↔ Ag(s) ; [Ag+] = 1.55 × 10−4 M E0 = 0.7994 V 1.03 V 1.12 V 1.24 V 0.36 V
For the cell shown, the measured cell potential, E cell, is -0.3643 V at 25 °C. Pt(s) | H₂(g,0.895 atm) | H* (aq, ? M) || Cd² +(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are → H₂ (g) 2 H+ (aq) + 2 e [H+] Cd²+(aq) + 2e Calculate the H+ concentration. = 0.141 → Cd(s) Incorrect E° = 0.00 V Eº = -0.403 V M
Consider a galvanic cell based on the reaction 2 Fe2+ (aq) + Cl2 (g) ------------>2 Fe3+ (g) + 2Cl- (aq) Calculate the cell potential at 25oC when [Fe2+ ] =1.0 M, [Fe3+ ] = 1.0 x 10-3 M, [Cl- ] = 3.0 x 10-3 M and PCl2 = 0.50 atm.
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Sn] = 0.0595 M, [Co1 = 0.0452 M, [Sn+] = 0.00261 M, and [Co*] = 0.00954 M. Standard reduction potentials can be found in %3D %3D this table. Sn (aq) + 2 Co+(aq) Sn+(aq) +2 Co*(aq) V E =
Consider the same diagram of a galvanic cell as in previous question, where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Ni2+(aq) + 2e– --> Ni(s); Eo = – 0.23 V What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M. (A) 1.15 V (B) 1.30 V (C) 0.76 V (D) 0.91 V
What is the standard cell potential for the voltaic (galvanic) cell using the following half-cell reactions with the indicated standard half-cell potentials: Be²⁺(aq) + 2e⁻→Be(s), E⁰ = -2.9V and Cl₂ + 2e⁻→2Cl⁻(aq), E⁰= +1.4 V A) -1.5 V B) +1.5 V C) -4.3 V D) 4.3 V
Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is 1.120 V at 25oC. Ni(s) | Ni2+(aq) ( ? M) || Ag+(aq) (0.84 M) | Ag(s) Ni2+(aq) + 2 e- → Ni(s) Eo = -0.257 V Ag+(aq) + e- → Ag(s) Eo = 0.800 V Your answer should have 2 significant figures.
For the cell reaction, Zn(s) | Zn2+(aq, 1 M) || Cu²*(aq, 1 M) | Cu(s), the electrode potential of cathode and anode are 0.34 V and -0.76 V respectively, what is the cell potential? O 1.10 V O -0.42 V O -1.10 V O 0.42 V
I have solved this equation and seen solutions to it. However, I keep seeing Pb2+ squared in the Nernst Equation (for Q) for the calcuation of the second part of this question. I do not understand why Pb2+ is squared. Can you explain that to me? Thank you.
A voltaic cell is being constructed from an Al/A|^ 3+ electrode and a Sn/Sn^ 2+ electrodeWhen constructed properly and the circuit is closed, the tin electrode is observed to gain mass and the overall cell potential to be 1.52V. Which of the following chemical reactions takes place at the cathode? Al3+(aq) + 3e- → Al(s) Sn(s) → Sn2+(aq) + 2e- Sn2+(aq) + 2e- → Sn(s) Al(s) → Al3+(aq) + 3e- Based on the overall reaction taking place across the voltaic cell, how many moles of electrons are involved? When electrons are flowing in the cell, which electrode gains mass? True or false: If an aluminum electrode is set to be part of a voltaic cell that also involves a standard hydrogen electrode (SHE), the aluminum electrode would be the anode.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V ʼred MnO,(aq)+2 H,O(1)+3e MnO,(s)+4 ОН (аq) E=+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.