Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If E^o cathode =...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If E^o cathode = 0.579 V and E^o anode = 1.152 V, and [N2+(aq)] = 0.115 M and [M+(aq)] = 0.022 M, what is E cell, using the Nernst equation? ____ V Provide your response to two digits after the decimal.
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Consider the galvanic cell described by (N and M are metals):
N(s)|N2+(aq)||M+(aq)|M(s) If E^o cathode =...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.585...
Consider the galvanic cell described by (N and M are
metals):
N(s)|N2+(aq)||M+(aq)|M(s)
If Eocathode = 0.585 V and
Eoanode = 1.27 V, and
[N2+(aq)] = 0.22 M and [M+(aq)] = 0.475 M,
what is Ecell, using the Nernst equation? ____
V
Provide your response to two digits after the decimal.
Question 1 1 pts Consider the galvanic cell described by (N and Mare metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eºcathode = 0.585 V and Eanode = 1.27 V, and [N2+(aq)] = 0.22 M...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.93 V and Eoano...
Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eocathode = 0.93 V and Eoanode = 1.814 V, and [N2+(aq)] = 0.568 M and [M+(aq)] = 0.299 M, what is Ecell, using the Nernst equation? ____ V Provide your response to two digits after the decimal.
urgent thank you Consider the galvanic cell shown below of Cr/Cr(aq) anode and an 12/1" (aq)...
urgent thank you
Consider the galvanic cell shown below of Cr/Cr(aq) anode and an 12/1" (aq) (Pt) cathode. The standard reduction potentials are as follows: C++ 3e -- Cr(s) E= 0.73 12(aq) + 2e - 21" E = +0.54 V Use the concentrations below to determine what is the value of E for this cell at 25°C? Cathode: 0.50 M 12/0.10M I Anode: 0.20 M C+ Select one: a. 1.34 V b. 0.59 V 2.14 V d. 1.76 V 1.88...
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...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2:...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq)...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339...
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339 V (AD + 14H(aq) + 6e-4 2Cr 3+(aq) + 7 H2O(1) Eo=1.330 V a) Write the overall cell reaction and determine its voltage. b) If the E value of the galvanic cell is 1.2 le of the galvanic cell is 1.254 V, calculate the pH of the cell when [Cu2+]=0.00010 M, Cr-0,2-1=0.00460 M, Cr3+1=1.0x102 M. The Nerst equation is E=E - (0.0592/n)logQ
Consider the galvanic cell described by (N and M are
metals):
N(s)|N2+(aq)||M+(aq)|M(s)
If Eocathode = 0.585 V and
Eoanode = 1.27 V, and
[N2+(aq)] = 0.22 M and [M+(aq)] = 0.475 M,
what is Ecell, using the Nernst equation? ____
V
Provide your response to two digits after the decimal.
Question 1 1 pts Consider the galvanic cell described by (N and Mare metals): N(s)|N2+(aq)||M+(aq)|M(s) If Eºcathode = 0.585 V and Eanode = 1.27 V, and [N2+(aq)] = 0.22 M...
urgent thank you
Consider the galvanic cell shown below of Cr/Cr(aq) anode and an 12/1" (aq) (Pt) cathode. The standard reduction potentials are as follows: C++ 3e -- Cr(s) E= 0.73 12(aq) + 2e - 21" E = +0.54 V Use the concentrations below to determine what is the value of E for this cell at 25°C? Cathode: 0.50 M 12/0.10M I Anode: 0.20 M C+ Select one: a. 1.34 V b. 0.59 V 2.14 V d. 1.76 V 1.88...
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...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339 V (AD + 14H(aq) + 6e-4 2Cr 3+(aq) + 7 H2O(1) Eo=1.330 V a) Write the overall cell reaction and determine its voltage. b) If the E value of the galvanic cell is 1.2 le of the galvanic cell is 1.254 V, calculate the pH of the cell when [Cu2+]=0.00010 M, Cr-0,2-1=0.00460 M, Cr3+1=1.0x102 M. The Nerst equation is E=E - (0.0592/n)logQ
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