voltaic cell is constructed from a standard g2+ Hg half cell (E° 855V) and a standard F half cell (E° red 870V). Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) me anode reaction is: + ↑ + he cathode reaction is: + → he spontaneous cell reaction is: + he cell voltage is V. ↑ + +

voltaic cell is constructed from a standard g2+ Hg half cell (E° 855V) and a standard F half cell (E° red 870V). Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) me anode reaction is: + ↑ + he cathode reaction is: + → he spontaneous cell reaction is: + he cell voltage is 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

A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb+2 half cell. All solutions are 1.0 M. Ag+(aq) + e- → Ag(s) E° = 0.80 V Pb+2(aq) + 2e- → Pb(s) E° = -0.13 V a.Diagram the cell, labeling electrodes and solutions, show the direction of electron flow in the circuit and what occurs in the salt bridge. b. If the cell were made with [Pb+2] = 0.10 M and [Ag3+] = 3.0 M, would the voltage increase, decrease, or remain the same? Explain using Q. c.Identify the electrode that is gaining mass
A voltaic cell is constructed based on the following pair of half-reactions. Identify the components in the cell below.Ag+(aq)+1e−Ag(s)Eo= 0.7996 VCd2+(aq)+2e−Cd(s)Eo= -0.403 V Write the the overall balanced equation, inluding states of matter.
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
A voltaic cell is constructed in which the anode is a Ni|Ni2+ half cell and the cathode is a Hg|Hg2+ 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 Ni|Ni2+ electrode the Hg|Hg2+ electrode.In the salt bridge, anions migrate the Hg|Hg2+ compartment the Ni|Ni2+ compartment.
A voltaic cell is constructed in which the anode is a Al|Al3+ half cell and the cathode is a H2|H+ 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 H2|H+ electrode the Al|Al3+ electrode.In the salt bridge, anions migrate the Al|Al3+ compartment the H2|H+ compartment. Submit Answer Retry Entire Group 1 more group attempt remaining
-3 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in One half-cell in a voltaic cell is constructed from a copper wire electrode in a 3.9 x 10 a 0.45 M solution of Zn(NO3)2 . Calculate the cell potential. You may need to use the following data: Zn²+ (aq) + 2 e¯ → Zn(s) E° = -0.763 V Cu²+ (aq) + 2 e¯ → Cu(s) E° = +0.337 V Potential = V
A non-standard state galvanic cell is constructed at 25.00°C as described here. The Fe(s) anode is immersed in a 0.040 M Fe(NO3)2 solution. The Cu(s) cathode is immersed in a 0.0060 M Cu(NO3)2. The circuit is completed with a salt bridge containing 1.0 M KNO3. The standard Fe/Fe2+ reduction potential is –0.44 V. The standard Cu/Cu2+ reduction potential is +0.34 V. Calculate the non-standard-state cell potential for this galvanic cell and determine if the reaction described is spontaneous under these conditions.
Consider the electrolysis reactions cathode anode whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = Cu²+ (aq, 0.177 M) +2e=Cu(s) H₂O(1) ⇒ 10₂(g, 1 bar) + 2 H+ (aq, 0.195 M) + 2 e¯ The cell has a resistance of 66.0 and a current of 7.17 mA when the cathode overpotential is 0.231 V and the anode overpotential is 0.050 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Ecell = V V
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25.0 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
A voltaic cell is constructed in which the anode is a Mg|Mg2+ half cell and the cathode is a Pb/Pb2+ 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 Pb|Pb2+ electrode In the salt bridge, anions migrate + from to ✓the Mg|Mg2+ compartment Enter electrons as e. the Mg|Mg2+ electrode. ✓the Pb|Pb²+ compartment.