36. A Voltaic cell is made from lead and manganese at standard state conditions. What happens to the lead and manganese electrodes over time? current Mn Anode Pb Cathode Reduction half-reaction Pb2+ (aq) + 2e → Pb(s) -0.13 V Mn2+(aq) + 2e → Mn(s) -1.18 V A) Nothing, this cell would not have spontaneous electron flow. B) The lead electrode would shrink over time and the manganese electrode would grow. C) The manganese electrode would shrink over time and the lead electrode would grow. D) Both electrodes would get larger over time. E) Both electrodes would shrink over time.

36. A Voltaic cell is made from lead and manganese at standard state conditions. What happens to the lead and manganese electrodes over time? current Mn Anode Pb Cathode Reduction half-reaction Pb2+ (aq) + 2e → Pb(s) -0.13 V Mn2+(aq) + 2e → Mn(s) -1.18 V A) Nothing, this cell would not have spontaneous electron flow. B) The lead electrode would shrink over time and the manganese electrode would grow. C) The manganese electrode would shrink over time and the lead electrode would grow. D) Both electrodes would get larger over time. E) Both electrodes would shrink over time.

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

Examine the galvanic cell below. Ni- www Volts 1.0.M t 1.0 M Ni (NO₂)₂ KNO 1 1.0 M AgNO₂ The reaction that occurs at the cathode is: Ni (s) → Ni²+ (aq) + 2e¯ ONi²+ (aq) + 2e → Ni (s) Ag+ (aq) + e¯ → Ag(s) Ag(s) → Ag+ (aq) + e- - Ag
Suppose the galvanic cell sketched below is powered by the following reaction: Mn(s)+ FeCl,(aq) → MnCl,(aq)+Fe(s) e- E1 E2 S1 S2
Sketch the voltaic cell for the following reaction. Identify what is being oxidized and what is being reduced.Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+ (aq)
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
2.Write a balanced cell reaction. Include the phases of all species in the chemical equation.
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
Analyze the components of a voltaic electrochemical cell. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Hg2+(aq) + Cu(s)→ Hg(I) + Cu²+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + + Enter the reaction that takes place at the cathode. Include state symbols: + + In the external circuit, electrons migrate to v the Hg+ electrode from v the Cu electrode. In the salt bridge, anions migrate to the Cu compartment [from v) the Hg compartment.
PART 2: Answer what is asked for each problem and show your solution. Round your answers to four decimal places and they must be enclosed all in a box. 1. Given the following reduction potentials: Ag*(aq) + e → Ag(s) Zn?"(aq) + 2e → Zn(s) Calculate the cell potential for the following reaction and predict whether the reaction will take place. If it will take place write the cell notation. Znº"(aq) + 2Ag(s)→ Zn(s) + 2Ag*(aq) E° = 0.80 V; E° = -0.76 V 2. A chromium metal was deposited coming from a solution of Cr*³. The amount of the said metal deposited weighs 2.19 g. The process is made possible through a current of 35.2 Amperes in electrolyte cell. Determine the following: a. How much charge (in C) is required? b. How long (in min) would it take for the reaction to occur?
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
Consider the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) What is the half-cell reaction for reduction? Multiple Choice О Fe(s) -> Fe2+(aq) + 2 e- Cu2+(aq) + 2 e-→ Cu(s) О Cu(s) → Cu2+(aq) + 2e- Fe(s) + 2 e-→ Fe2(aq)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction + 21O3(aq)+ 12 H¹ (aq)+10e¯ Cl₂(g) +2e 1₂(s) + 6H₂O(1) → 2 C1 (aq) standard reduction potential E=+1.195 V 'red E 70 = +1.359 V red
A particular voltaic cell operates on the reaction below, giving an emf of 0.853 V. Calculate the maximum electrical work (in kJ) generated when 20.2 g of zinc metal is consumed. Zn(s) + CI2(g) → Zn2+(aq) + 2 Cl −(aq)