Design a voltaic cell with the following two reduction half-reactions: Ag*(aq) + e-Ag(s) E° = 0.80 V Cu2*(aq) + 2 e → Cu(s) E° = 0.34 V Silver will be placed in the [Select ] and the sign for overall Ece° will be [Select] [ Select Negative Positive

Design a voltaic cell with the following two reduction half-reactions: Ag(aq) + e-Ag(s) E° = 0.80 V Cu2(aq) + 2 e → Cu(s) E° = 0.34 V Silver will be placed in the [Select ] and the sign for overall Ece° will be [Select] [ Select Negative Positive

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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Consider the following voltaic cell reaction at 25 °C. 2Ag (aq) + Ni(s) → Ni2*(aq) + 2Ag(s) Calculate [Ag* when [Ni2*] = 1.0 × 104 M, Ecel = 1.17 V, and E°cell = 1.06 V for this reaction. Ecell = E° 0.0592 V Jog Q cell O 0.72 M O 0.085 M O 0.52 M O 1.4 x 10-4M
If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter? Half-Reaction E° (V)   Zn2+(aq) + 2e–→ Zn(s) –0.76     Ag+(aq) + e–→Ag(s) +0.80   Question 6 options: -0.04 V 0.04 V 2.36 V 1.56 V -2.36 V
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
2req A voltaic cell is constructed from a standard Sn*Sn half cell (Eo 2+ -0.140V) and a standard Cr* Cr half cell (E red red =-0.740V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) 2req The anode reaction is: s 2req OMD The cathode reaction is: OM) s 2req OMD The spontaneous cell reaction is: ts 2req OM) ts The cell voltage is V.
Use the standard reduction potentials given below to predict if a reaction will occur between Sn(s) and I2 (s), when the two are brought in contact via standard half-cells in a voltaic cell. I₂ (s) + 2e¯ → 21¯(aq) E red Sn²+ (aq) + 2e¯ → Sn(s) Fº red = = 0.535 V + -0.140 V If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
14. Determine overall E° cell for the voltaic cell and diagram the cell including the anode, cathode, movement of electrons, and the KNO3 salt bridge: → Ag (s) Eo = +0.80 V 1+ Ag "(aa) e- E° = - 0.74 V !! Cr 3+ (ag) + 3e → Cr (8)
consider a voltaic cell with the overall reaction zn + 2ag+ zn2+ + 2ag what will the value of e cell (v) be when [ag+] =1.9 m and zn 2+ = .003m Ag^+ + e- -> Ag(s). E red = 0.80V zn2^+ + 2e^- -> Zn (s) E red = -0.76 V
2. What is the value of E° cell for the following electrochemical reaction? Use the table of standard reduction potentials provided with the Ch 16 Notes to solve. Fe3+ (aq) + Li (s) → Fe²* (aq) + Li*(aq)
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.
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.
Design a voltaic cell given the reduction half reactions below then give the electrochemical cell notation below to describe the cell. NO3 (aq) + 4 H* (aq) + 3 e --> NO (g) + 2 H20 (1) Cu2* (aq) + 2 e --> Cu (s)
The standard reduction reactions for the two metals are listed below Sn (aq)+2eSn(s) E 0.14 V A (aq) + 3e' --> Alls) E=-1.66 V Type a proper balanced chemical equation for the above reaction if an electrochemical cell were to be constructed. Use the same symbolism in the question. This include (aq). (s), and For superscripts you can type regular numbers but use the appropriate charges. Example for Na(s) and X(s): Na1+(aq) + X(s) --> X1+(aq) + Na(s) Notice where spaces are in the example equation. If coefficients are needed do not put a space between the coefficient and the metal or ion species.