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For a galvanic cell where the standard free energy change is negative and the cell potential...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
A ______ value for Gibbs free energy corresponds to a _____ value for cell potential and results in a _______ reaction....
A ______ value for Gibbs free energy corresponds to a _____ value for cell potential and results in a _______ reaction. a. positive, positive, spontaneous b. positive, negative, spontaneous c. positive, positive, nonspontaneous d. positive, negative, nonspontaneous
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
Suppose the Gibbs free energy change of a reaction has a large positive value. What does...
Suppose the Gibbs free energy change of a reaction has a large positive value. What does this say about the spontaneity of the chemical reaction? Select the correct answer below: O The chemical reaction is spontaneous. O The chemical reaction is not spontaneous. O The Gibbs free energy change, in itself, says nothing about whether a reaction is spontaneous O There is not enough information provided for a definitive answer
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is...
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V. Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -679 kJ and ΔS∘ = -195 J/K .
DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state)...
DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state) for the reaction below is -8.6 kJ/mol. What is ao for this reaction at 37°C when [A)-0.2 M [B-0.2 M, (C]-0.4 M, and ID)-0.6 M? ABCDase A BCD 3.98 J/mol O -4.16 KJ/mol 0-13.22kJ/mol 0 6.81k/moll DI Question 4 2 pts Which one of the following statements is true? 0 if ΔG is negative, the reaction will be spontaneous. Exothermic reactions are always spontaneous....
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which i...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Cd(II) and Sc(III) Cathode: Cd(II) Sc(III) Anode: Cd(II) Sc(III) Ecell 42 (b) Pb(II) and In(III) Cathode: Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: Ni(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell- Supporting Materials We were unable to transcribe this imageAGº and Eº can...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Question 7 (1 point) Calculate the standard free energy for the following reaction at standard conditions....
Question 7 (1 point) Calculate the standard free energy for the following reaction at standard conditions. Will the galvanic cell occur spontaneously to produce potential? Cu (s) + V2+ (aq) - Cu2+ (aq) + V (s) O + 148 kJ, the reaction will not be spontaneous + 295 kJ, the reaction will not be spontaneous - 148 kJ, the reaction will occur spontaneously as written 295 kJ, the reaction will occur spontaneously as written Show Report e STRAIN605 PASSW lenovo
Using tabulated standard reduction potentials from your text, calculate the standard cell potential, E degree_cell (always...
Using tabulated standard reduction potentials from your text, calculate the standard cell potential, E degree_cell (always positive for a galvanic cell), based on the following reaction: Cu^2+ (aq) + Mg(s) Mg^2+ (aq) + Cu(s) A galvanic cell based on the above reaction is constructed according to the generic sketch of a galvanic cell shown below:
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
Suppose the Gibbs free energy change of a reaction has a large positive value. What does this say about the spontaneity of the chemical reaction? Select the correct answer below: O The chemical reaction is spontaneous. O The chemical reaction is not spontaneous. O The Gibbs free energy change, in itself, says nothing about whether a reaction is spontaneous O There is not enough information provided for a definitive answer
DI Question 3 2 pts The AG (change in Gibbs free energy at standard biochemical state) for the reaction below is -8.6 kJ/mol. What is ao for this reaction at 37°C when [A)-0.2 M [B-0.2 M, (C]-0.4 M, and ID)-0.6 M? ABCDase A BCD 3.98 J/mol O -4.16 KJ/mol 0-13.22kJ/mol 0 6.81k/moll DI Question 4 2 pts Which one of the following statements is true? 0 if ΔG is negative, the reaction will be spontaneous. Exothermic reactions are always spontaneous....
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Cd(II) and Sc(III) Cathode: Cd(II) Sc(III) Anode: Cd(II) Sc(III) Ecell 42 (b) Pb(II) and In(III) Cathode: Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: Ni(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell- Supporting Materials We were unable to transcribe this imageAGº and Eº can...
Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential. (Use the table of Standard Electrode Potentials.) (a) Ca(II) and Sc(III) Cathode: . Ca(II) Sc(III) Anode: Ca(II) Sc(III) Ecell = 0.0591 x V (b) Pb(II) and In(III) Cathode: . Pb(II) In(III) Anode: Pb(II) In(III) Ecell - (c) Ni(II) and Zr(IV) Cathode: NI(II) Zr(IV) Anode: Ni(II) Zr(IV) Ecell - V Supporting Materials Periodic Table Supplemental...
Question 7 (1 point) Calculate the standard free energy for the following reaction at standard conditions. Will the galvanic cell occur spontaneously to produce potential? Cu (s) + V2+ (aq) - Cu2+ (aq) + V (s) O + 148 kJ, the reaction will not be spontaneous + 295 kJ, the reaction will not be spontaneous - 148 kJ, the reaction will occur spontaneously as written 295 kJ, the reaction will occur spontaneously as written Show Report e STRAIN605 PASSW lenovo
Using tabulated standard reduction potentials from your text, calculate the standard cell potential, E degree_cell (always positive for a galvanic cell), based on the following reaction: Cu^2+ (aq) + Mg(s) Mg^2+ (aq) + Cu(s) A galvanic cell based on the above reaction is constructed according to the generic sketch of a galvanic cell shown below:
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