A voltaic cell is constructed from a standard Pb2+ Pb half cell (E° red = -0.126V) and a standard I2I half cell (E° red 0.535V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Previous +

A voltaic cell is constructed from a standard Pb2+ Pb half cell (E° red = -0.126V) and a standard I2I half cell (E° red 0.535V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Previous +

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...

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A voltaic cell is constructed from a standard Cd2+|Cd half cell (E°red = -0.403V) and a standard Br2|Br- half cell (E°red = 1.080V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.
Give the balanced cell equation and determine & for the galvanic cells based on the following half-reactions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H₂O2 + 2H+ + 2e → 2H₂O € = 1.78 V Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V a. b. € = V € = + 2H+ + 2e → H₂ → Al A1³+ +3e V € = 0.00 V € = -1.66 V
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0)
Enter electrons as e A voltaic cell is constructed from a standard Zn2+ Zn half cell (E°red= -0.763V) and a standard Br₂ Bri half cell (Ered 1.080V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is Submit Answer (sky Another Vorstan
A voltaic cell is constructed from a standard Zn2+|Zn half cell (E°red = -0.763V) and a standard Ag+|Ag half cell (E°red = 0.799V). The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.
Consider a galvanic cell at T = 298K. F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+] = 2M. Consider the half-reactions below: Ca2+(aq) + 2e- → Ca(s) E0red = - 2.76 V HfO2+(aq) + 2H+(aq) + 4e- → Hf(s) + H2O(l) E0red = -1.72 V a. Find the general reaction, E0cell, and identify the cathode and the anode. Indicate the direction of the flow of electrons (from which solid plate to the other solid plate). b. Write the line notation for this cell. c. Find ΔG0. *d. Express and calculate Q (at t0) e. Express and calculate K. f. What value do you expect for Ecell at this point? Why? g. Find Ecell (at t0) After a certain period of time (t1), the H+ concentration is one-fifth of its initial concentration. *h. Do the RICE and find the concentrations of all species at t1 i. Find the pH at t1 in two…
A voltaic cell is constructed from a standard Ag+ | Ag half cell (E° red = .799V) and a standard Br2 | Br- half cell (E° red = 1.080V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is V.
A voltaic cell is constructed from a standard Zn2+ | Zn half cell (E°red = -0.763 V) and a standard Br2 | Br- half cell (E°red = 1.080 V). (For all reactions below, use the smallest possible integer coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. Enter electrons as .) The anode reaction is: + + The cathode reaction is: + + The spontaneous cell reaction is: + + The cell voltage is ______ V.
Enter electrons as e A voltaic cell is constructed in which the anode is a Fe2+|Fe3+ half cell and the cathode is a F|F, half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: +. In the external circuit, electrons migrate the Fe2+|Fe3+ electrode the F|F, electrode. from to In the salt bridge, anions migrate the F|F, compartment 3- the Fe2+|Fe+ compartment. +. +. 1
A voltaic cell is constructed from a standard Cr+ Cr half cell (E°red = -0.740V) and a standard F2F half cell (E°. red = 2.870V). (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.) The anode reaction is: per) Greek(lower) Arrows Other The cathode reaction is: + elp The spontaneous cell reaction is: The cell voltage is V.
Enter electrons as e". Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. I(s) + Ni(s) → 21°(aq) + Ni²*(aq) The anode reaction is: The cathode reaction is: In the external circuit, electrons migrate V the NiNi2+ electrode the I12 electrode. v the Ni|Ni* compartment In the salt bridge, anions migrate| |I, compartment. the I + +
A voltaic cell is constructed from a standard Al³+|Al half cell (E° red = -1.660V) and a standard Sn²+ | Sn half cell (Eºred = -0.140V). The anode reaction is: + The cathode reaction is: + Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. The spontaneous cell reaction is: + The cell voltage is - V. + + +