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? Cu²+(aq) + 2e –→ Cu(s); E=0.34 V Cr3+ (aq) + 3e - Cr(s); E=-0.74 V Oa. Chromium, 1.08 V Ob. Copper, -0.4 V Oc. Copper, 0.40 V Od. None of the other options Oe. Chromium, 0.40 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? Cu²+(aq) + 2e –→ Cu(s); E=0.34 V Cr3+ (aq) + 3e - Cr(s); E=-0.74 V Oa. Chromium, 1.08 V Ob. Copper, -0.4 V Oc. Copper, 0.40 V Od. None of the other options Oe. Chromium, 0.40 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

Given the cell reaction, Zn(s) + Cut2(a the cathode in the cell is: Cu(s) Cu +2 OPt (aq) Zn(s) +2 (aq) → Zn¹2(aq) + Cu(s) +2 Zn (aq)
A chemist designs a galvanic cell from the following two half-reactions Ered = +0.96 V NO3(aq) + 4H+ (aq) + 3e¯ → NO(g) + 2H₂O (1) Ered +0.153 V Cu²+ (aq) + e¯ → Cut (aq) The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] = V.
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
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
12 The standard cell potential for the following galvanic cell is 0.71 V. Mg(s) Mg2+(aq)||A13+(aq)|Al This reaction has an equilibrium constant, K =
Sn(s) | Sn2+ (aq, 1.8 M) || Agt(aq, 0.055 M) | Ag(s) Consider the cell notation of a galvanic cell given above and the following reduction potentials: Sn- (aq) + 2e- → Sn(s) E° = -0.14 V Ag (aq) + e- → Agis) ED=0.80 V 1. The number of electron transferred in the net reaction is [Select] 2. The E is [Select] 3. The value for Q is (Select] 4. The cell potential for the cell is [Select] V.
4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
Write a balanced equation for the overall cell reaction in the following galvanic cell and tell why inert electrodes are required at the anode and cathode. Pt(s) | Br (aq) | Br₂ (1) || Cl; (g) | Cl(aq) | Pt(s)
Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Cd²+] = 0.00100 M and [Au*] = 0.795 M. Standard reduction potentials can be found in this table. 3 Cd(s) + 2 Au³+(aq) =3 Ca²*(aq) + 2 Au(s) 1.81 E = Incorrect
The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard conditions. Zn(s) + Cu2+(aq) => Cu(S) + Zn2+(aq) What is the cell potential when one of the following deviations from standard conditions are made? A) [Zn2+] = 0.25 M; [Cu2+] = 0.25 M B) [Zn2+] = 0.25 M; [Cu2+] = 0.50 M C) [Zn2+] = 0.75 M; [Cu2+] = 0.75 M D) [Zn2+] = 0.75 M; [Cu2+] = 0.25 M E) [Zn2+] = 0.25 M; [Cu2+] = 0.75 M