Volt- meter Wire Cd- Ag Salt Bridge (1 M Cd(NO3)2 100 milliliters 1 M AgNO3 100 millilitersi The spontaneous reaction that occurs when the cell above operates is: 2Ag* + Cd(s) -> 2 Ag(s) + Cd- Use the diagram above and the balanced equation, and choose which result will occur as a result of the following change. The salt bridge is replaced by a platinum wire a Voltage increases. O b Voltage decreases. Voltage becomes zero and remains at zero. O d No change in voltage occurs. O e ) Direction of voltage change cannot be predicted without additional information.

Volt- meter Wire Cd- Ag Salt Bridge (1 M Cd(NO3)2 100 milliliters 1 M AgNO3 100 millilitersi The spontaneous reaction that occurs when the cell above operates is: 2Ag* + Cd(s) -> 2 Ag(s) + Cd- Use the diagram above and the balanced equation, and choose which result will occur as a result of the following change. The salt bridge is replaced by a platinum wire a Voltage increases. O b Voltage decreases. Voltage becomes zero and remains at zero. O d No change in voltage occurs. O e ) Direction of voltage change cannot be predicted without additional information.

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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Number 2
Write the galvanic cell notation and E°rxn of the following , use the information given below as needed Metals Cell Notation for a Galvanic Cell E°rxn Ni-Cd Ni-Sn Sn-Cd Sn-Pb Fe-Sn Fe-Pb Ag-Pb Cu-Pb Ag-Zn half Reactions Std E° Mg2+ (aq) + 2e- à Mg(s) -2.370 Zn2+ (aq) + 2e- à Zn(s) -0.763 Fe2+ (aq) + 2e- à Fe(s) -0.440 Cd2+ (aq) + 2e- à Cd(s) -0.402 Ni2+ (aq) + 2e- à Ni(s) -0.250 Sn2+ (aq) + 2e- à Sn(s) -0.140 Pb2+ (aq) + 2e- à Pb(s) -0.126 Cu2+ (aq) + 2e- à Cu(s) +0.339 Ag+ (aq) + e- à Ag(s) +0.799
For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn² (0.25M) mixed with Cu and Cu2 (0.35M)
Consider a galvanic cell based in the reaction Fe2+ + Cr,O,→ Fe³+ + Cr³* . Cr,03- + 14H* + 6e¯ →2Cr+ + 7H,0 1.33 Fe+ + e→ Fe?+ 0.77 Balance the reaction. What is the coefficient of Fe3+ in the balanced equation? а. 3 b. 6 с. 4 d. 2 e. none of these
What is Eo for the spontaneous cell that contains the following half-reaction? Cu2+ + 2e1- --> Cu Eo=0.34 V Fe2+ + 2e1- --> Fe Eo=-0.44 V
In Electrochemical cells electrons are transfered from the reactants being reduced to the reactants being oxidized through a wire connecting the two containers. (True/False)
Using the reduction half-reactions in the table below, write a balanced net-ionic equation representing the overall reaction that takes place as the cell operates.
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? ______V (b) What is the emf of this cell when [Ce4+] = 2.0 M, [Ce3+] = 0.012 M, and [Cr3+] = 0.011 M? _______V (c) What is the emf of the cell when [Ce4+] = 0.58 M, [Ce3+] = 0.88 M, and [Cr3+] = 1.2 M? _______V
Consider a galvanic cell created from the following redox reaction: 3Zn (s) + 2Au3+ (aq) → 3Zn2+ (aq) + 2Au (s) 1) Draw out a schematic diagram (as shown in image) 2) Label each component (anode, cathode, salt bridge, solution choice, and electron flow direction) in your schematic diagram.
a)Which redox reaction is not spontaneous under standard conditions? a 2 Fe + 3 Br2 → 2 Fe3+ + 6 Br− b 2 Fe3+ + 3 Ni → 2 Fe + 3 Ni2+ c Fe2+ + Ni → Fe + Ni2+ d 2 Fe3+ + Ni → 2 Fe2+ + Ni2+ e All of the above reactions are spontaneous b)Consider the following half-reaction: BrO- → Br- The balanced equation for the half-reaction in basic conditions is: a BrO- + 2H+ + 2e- → Br- + H2O b BrO- + 2H+ → Br- + H2O + 2e- c BrO- + H2O → Br- + 2OH- + 2e- d BrO- + H2O + 2e- → Br- + 2OH-
Chemistry Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Write the balanced equation for the overall reaction in acidic solution.