2. Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Zn(s) + Cu2+(aq) à Zn2+(aq) + Cu(s)
E°red = -0.763 V for Zn2+(aq) + 2e- à Zn(s)
E°red = +0.340 V for Cu2+(aq) + 2e- à Cu(s)
3. What is the ∆G°rxn for a 2 electron transfer electrochemical cell with a standard cell potential of +0.770 V.
4. Based on the following reduction potential data, what is the ∆G°rxn for the following electrochemical cell reaction: Zn(s) + Cu2+(aq) à Zn2+(aq) + Cu(s)?
E°red = -0.763 V for Zn2+(aq) + 2e- à Zn(s)
E°red = +0.340 V for Cu2+(aq) + 2e- à Cu(s)
5. Which of the following acids is a strong oxidant?
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Question 8 3.03 pts Based on the following reduction potential data, what is the AGºran for the following electrochemical cell reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)? Eres -0.763 V for Zn2+ (aq) + 2e - Zn(s) Ered = +0.340 V for Cu2+(aq) + 2e - Cu(s) O +106 kJ/mol O-106 kJ/mol -213 kJ/mol
+ Calculate the change in the standard free energy for the following reaction: Zn + Cu?+ Zn²+ (aq) + Cu (3) Standard Reduction Potentials (5) (aq) + 2e → = -0.763 V (aq) + 2e → Cu (s) Ered = 0.337 V (aq) → → Zn (5) Ered Zn2+ Cu2+ A. - 212 kJ/mol B. 175 kJ/mol C. 81.0 kJ /mol OD. - 106 kJ / mol
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Zn -0.763 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A Part complete In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the...
Using the information in the table: Which combination of metals, if used to create an electrochemical cell, would produce the largest voltage? Liu lur the reaction between Zn and Cu2+ ions is 1.1030 V, we can use the known value for the half-cell potential for zinc to determine the half-cell potential for copper: Zn(s) → Zn2+(aq) + 2e + Cu2+(aq) + 2e → Cu(s) Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) E half-cell = 0.7628 V Eºhalf-cell =...
Find the best combination of half-cell pair from the following list, which will give the highest voltage. What is the voltage for that Galvanic cell? Given that Reduction Half-reaction Standard Potential (Eredo) Zn2+(aq) + 2e– → Zn(s) -0.763 (V) Fe2+(aq) + 2e– → Fe(s) -0.44 (V) Cu2+(aq) + 2e– → Cu(s) +0.34 (V) Sn2+(aq) + 2e– → Sn(s) -0.14 (V) Cu2+(aq) + e– → Cu+(aq) + 0.153 (V) Ag+(aq) + e– → Ag(s) + 0.80 (V) Cu+(aq) + e– →...
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Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What is the cell potential of the following electrochemical cell at 25°C? Zn(s) | Zn2+(1.0 M) || Cu2+(0.0010 M) Cu(s) a) greater than 1.10 v b) between 0.76 and 1.10 V c) less than 0.42 V d) between 0.00 and 0.76 V e) between 0.34 and 0.76 V
Using the standard reduction potentials given below, choose the reaction than can only be achieved through electrolysis. Cu2+(aq) + 2e → Cu(s) E° = 0.34 V Pb2+(aq) + 2e + Pb(s) E° = -0.13 V Fe2+(aq) + 2e Fe(s) E° = -0.44 V Zn2+(aq) + 2e + Zn(s) E° = -0.77 V Zn2+(aq) + Pb(s) → Zn(s) + Pb2+(aq) o Fe2+(aq) + Zn(s) → Fe(s) + Zn2+(aq) Pb2+(aq) + Fe(s) → Pb(s) + Fe2+(aq) Cu2+(aq) + Fe(s) → Cu(s) +...
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
For the following cell what is the cell potential under standard conditions? Zn + Cu2+ → Cu + Zn2+ If Cu2+ + 2e- → Cu E° = 0.34V and Zn2+ + 2e- → Zn E° = -0.76 V