Using a table of reduction potentials from our lecture textbook, find a species that would pair well with an iron electr...
Using a table of reduction potentials from our lecture textbook, find a species that would pair well with an iron electrode (Fe?Fe3+) to form a spontaneous reaction. What would E0Cell for this voltaic be?
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Using a table of reduction potentials from our lecture textbook, find a species that would pair well with an iron electr...
1. Using a table of reduction potentials from your lecture textbook. Find a species that would pair well with an ir...
1. Using a table of reduction potentials from your lecture textbook. Find a species that would pair well with an iron electrode (Fe/Fe") to form a spontaneous reaction. What would Eºcell for this voltaic cell. 2. Using your own words, equate the Eºcell of a voltaic cell to AG (Gibb's free energy). How are they similar? Draw a schematic if necessary. 3. List two different possible experimental errors that could have led to the error in your calibration curve. How...
Standard potentials are measured against the standard hydrogen electrode (SHE). Because it is not...
Standard potentials are measured against the standard hydrogen electrode (SHE). Because it is not always convenient to use a S.Н.Е., often other reference electrodes are used. The saturated calomel electrode (SCE.) is one commonly used reference electrode, with a reduction potential of +0.242 V versus the S.H.E. Using a table of standard reductions, determine what the standard reduction potential of each reduction half-reaction would be versus the S.C.E Cl2 (g) + 2e-→ 2 Cl-(aq) E1.36 Fe3 + (aq) + 3...
The following are a selection of standard reduction potentials. Use this table to answer 418 (1)...
The following are a selection of standard reduction potentials. Use this table to answer 418 (1) 24" (aq) + 2e → Hz(g) 0.00 V (ii) Fe" (aq) + e + Fe (aq) +0.77 V (iii) Zn" (aq) +2e → Zn(s) -0.76 V (iv) Au (aq) + → Au(s) +1.50 V (v) Cl:(g) + 2e2 (aq) +1.36 V (vi) 1:(s) + 2e → 2(aq) +0.54 V (vii) Br_(l) +2e → 2Br (aq) +1.08 V (viii) Ni?" (aq) + 2e Ni(s) -0.25...
Question 40 (1 point) Consulting the table of standard reduction potentials provided, which species is the...
Question 40 (1 point) Consulting the table of standard reduction potentials provided, which species is the best oxidizing agent? 12 reaction Ered (V) Pb4+ + 2e → Pb2+ +1.67 Cd2+ + 2e Cd -0.40 OCd O Pb2+ OP64+ O ca²+ Question 39 (1 point) Which balanced equation corresponds to the formation reaction for carbon monoxide, CO(g)? CO(g) + 1202(g) → CO2(g) 2CO(g) + O2(g) → 2CO2(g) C(s) + 102(g) → CO(g) 2C(s) + O2(g) → 2CO(g) Question 38 (1 point)...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9 (online material), determine the standard free energy (AG) for the following reaction in kJ/mol. [Faraday constant = 96.5 kJ/V] [10 points) FADH2 + 1/202 - FAD + 2H+ + H:0 Show detailed calculation. Final answer without clear work will not be considered. TABLE 9.1 Standard Reduction Potentials Redox Half-Reaction 2H+ + 2e" - H a-Ketoglutarate + CO, + 2H+ 2e isocitrate NADP+ + H+...
both questions please! :) 15. Based on the table of standard reduction potentials in your OpenStax...
both questions please! :)
15. Based on the table of standard reduction potentials in your OpenStax textbook (table 16.1), what would be an appropriate cathode if solid silver was used as the anode? Calculate Eºcell for your chosen cathode. (6 pts) 16. A+B+C+D Imagine that you are performing kinetics studies on the above reaction. You vary the concentration of reagent A over multiple trials but find that it does not affect the time for the reaction to be completed. What...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
Using data table 3, can you help me with 3) Thank you. angement of reduction potentials...
Using data table 3, can you help me with 3)
Thank you.
angement of reduction potentials an increasing order (include reduction potential of the Copper electrode) Data Table 3 Half-Cell Reaction 1 Mars) → ng 2 +2é 1. Znow → Zn 2 + 2 € Snrs) → Jn 2 Tag + 2 é e(s) Fe2 Tag) + 2e- 18 Pb(s) Pb2 y + 2€ 18. Ales → AB Tagu +36 Er -1.18 -769 - 595 -,28 - 149 -,072 high...
Using the table of reduction potentials (Eo) for the half-reactions shown, match the given redox reactions...
Using the table of reduction potentials (Eo) for the half-reactions shown, match the given redox reactions with their Eo and predict the change in free energy by stating whether the reactions will be exergonic or endergonic Exergonic 1.14 V 1.00 V 0.15 V 1.24 V 1.24 V Endergonic Reaction Free Energy Eo (Volts) CO2/glucose [-0.43] -0.5 -0.4 NAD /NADH 0.32 -0.3 NADH H 12 OH.ONAD 2HH2 -0.42] CO2/methanol [-0.38] Co2/acetate [-0.28] FADFADH2[-0.18] Pyruvatelactate [-0.19] 6CO, + 6H,O → 60, +...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
1. Using a table of reduction potentials from your lecture textbook. Find a species that would pair well with an iron electrode (Fe/Fe") to form a spontaneous reaction. What would Eºcell for this voltaic cell. 2. Using your own words, equate the Eºcell of a voltaic cell to AG (Gibb's free energy). How are they similar? Draw a schematic if necessary. 3. List two different possible experimental errors that could have led to the error in your calibration curve. How...
Standard potentials are measured against the standard hydrogen electrode (SHE). Because it is not always convenient to use a S.Н.Е., often other reference electrodes are used. The saturated calomel electrode (SCE.) is one commonly used reference electrode, with a reduction potential of +0.242 V versus the S.H.E. Using a table of standard reductions, determine what the standard reduction potential of each reduction half-reaction would be versus the S.C.E Cl2 (g) + 2e-→ 2 Cl-(aq) E1.36 Fe3 + (aq) + 3...
The following are a selection of standard reduction potentials. Use this table to answer 418 (1) 24" (aq) + 2e → Hz(g) 0.00 V (ii) Fe" (aq) + e + Fe (aq) +0.77 V (iii) Zn" (aq) +2e → Zn(s) -0.76 V (iv) Au (aq) + → Au(s) +1.50 V (v) Cl:(g) + 2e2 (aq) +1.36 V (vi) 1:(s) + 2e → 2(aq) +0.54 V (vii) Br_(l) +2e → 2Br (aq) +1.08 V (viii) Ni?" (aq) + 2e Ni(s) -0.25...
Question 40 (1 point) Consulting the table of standard reduction potentials provided, which species is the best oxidizing agent? 12 reaction Ered (V) Pb4+ + 2e → Pb2+ +1.67 Cd2+ + 2e Cd -0.40 OCd O Pb2+ OP64+ O ca²+ Question 39 (1 point) Which balanced equation corresponds to the formation reaction for carbon monoxide, CO(g)? CO(g) + 1202(g) → CO2(g) 2CO(g) + O2(g) → 2CO2(g) C(s) + 102(g) → CO(g) 2C(s) + O2(g) → 2CO(g) Question 38 (1 point)...
Q7) Using Table 9.1 (page 294) in your textbook and/or in the slides of chapter 9 (online material), determine the standard free energy (AG) for the following reaction in kJ/mol. [Faraday constant = 96.5 kJ/V] [10 points) FADH2 + 1/202 - FAD + 2H+ + H:0 Show detailed calculation. Final answer without clear work will not be considered. TABLE 9.1 Standard Reduction Potentials Redox Half-Reaction 2H+ + 2e" - H a-Ketoglutarate + CO, + 2H+ 2e isocitrate NADP+ + H+...
both questions please! :)
15. Based on the table of standard reduction potentials in your OpenStax textbook (table 16.1), what would be an appropriate cathode if solid silver was used as the anode? Calculate Eºcell for your chosen cathode. (6 pts) 16. A+B+C+D Imagine that you are performing kinetics studies on the above reaction. You vary the concentration of reagent A over multiple trials but find that it does not affect the time for the reaction to be completed. What...
need help with the rest of the table
EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...
Using data table 3, can you help me with 3)
Thank you.
angement of reduction potentials an increasing order (include reduction potential of the Copper electrode) Data Table 3 Half-Cell Reaction 1 Mars) → ng 2 +2é 1. Znow → Zn 2 + 2 € Snrs) → Jn 2 Tag + 2 é e(s) Fe2 Tag) + 2e- 18 Pb(s) Pb2 y + 2€ 18. Ales → AB Tagu +36 Er -1.18 -769 - 595 -,28 - 149 -,072 high...
Using the table of reduction potentials (Eo) for the half-reactions shown, match the given redox reactions with their Eo and predict the change in free energy by stating whether the reactions will be exergonic or endergonic Exergonic 1.14 V 1.00 V 0.15 V 1.24 V 1.24 V Endergonic Reaction Free Energy Eo (Volts) CO2/glucose [-0.43] -0.5 -0.4 NAD /NADH 0.32 -0.3 NADH H 12 OH.ONAD 2HH2 -0.42] CO2/methanol [-0.38] Co2/acetate [-0.28] FADFADH2[-0.18] Pyruvatelactate [-0.19] 6CO, + 6H,O → 60, +...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
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