Homework Answers
![Znes) + 2H+ cag nth ag + H₂ (g) [zht 2] = IM Een 0,549 v PH = 1 atm E Zut2/2n = 0.76V EH1/4 = 0 (standard) E cell- E Cathole](http://img.homeworklib.com/questions/3ac50c60-30fa-11ec-9776-efbf380b8db5.png?x-oss-process=image/resize,w_560)
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Question 1 1 pts For the cell: Zn(s) + 2H+ (aq) + Zn2+(aq) + H2 (g)...
Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) +...
Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2(g) It is found that the voltage (think Ecell) is +0.560 V when [Zn2+1 -0.85 M and PH2 = = 0.988 atm. What is the pH in the H2-H half-cell?
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq)...
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq) | Pt,H2 (g) (P=1.00 atm) calculate DG° in kJ calculate Ecell for [H+] = 0.8 M and [Zn2+] = 0.5 M calculate K at 25°C
For a voltaic cell based on the reaction below, which statement is correct? Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) Zn2+(aq) is...
For a voltaic cell based on the reaction below, which statement is correct? Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) Zn2+(aq) is oxidized at the anode. H+(aq) is reduced at the cathode. Zn2+(aq) is reduced at the anode. H2(g) is the oxidizing agent.
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);...
Calculate Ho for the following equations: a. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)&n
Calculate Ho for the following equations: a. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g) b. 2H2S(g) + 3O2(g) 2SO2(g) + 2H2O(g) c. 3Ni(s) + 2NO3-(aq) + 8H+(aq) 3Ni2+(aq) + 2NO(g) + 4H2O(l)
If the potential of a Zn-H+ cell (see below) is 0.45 V at 25 C when...
If the potential of a Zn-H+ cell (see below) is 0.45 V at 25 C when the [Zn2+] = 1.0M and PH2 = 1 atm, what is the pH of the cathode solution? Zn(s)|Zn2+(aq)|| H+(aq)|H2 (g)|Pt
A galvanic cell was constructed with a Zn/Zn2+ half cell and an H2/H+ half cell(standard hydrogen...
A galvanic cell was constructed with a Zn/Zn2+ half cell and an H2/H+ half cell(standard hydrogen electrode, SHE). Calculate Ecell under the following conditions: [Zn2+] = 0.01 M, [H+] = 2.5 M, and PH2 = 0.30 atm at 25°C?
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq)...
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
Please include solutions, thank you. Consider the voltaic cell: Zn(s) + Cd2+(aq) → Zn2+ (aq) +...
Please include solutions, thank you.
Consider the voltaic cell: Zn(s) + Cd2+(aq) → Zn2+ (aq) + Cd(s). (Eºcell = 0.36V) operating at 319.351 K. If (conc. Cd2+) = 0.411 and (conc. Zn2+) = 1.101, calculate the Ecell (volts).
For the cell shown, the measured cell potential, ?cell, is −0.3629 V at 25 °C. Pt(s)...
For the cell shown, the measured cell potential, ?cell, is −0.3629 V at 25 °C. Pt(s) | H2(g,0.899 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g)?o=0.00 V Cd2+(aq)+2e−⟶Cd(s)?o=−0.403 V Calculate the H+ concentration. [H+]=
Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2(g) It is found that the voltage (think Ecell) is +0.560 V when [Zn2+1 -0.85 M and PH2 = = 0.988 atm. What is the pH in the H2-H half-cell?
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);...
Please include solutions, thank you.
Consider the voltaic cell: Zn(s) + Cd2+(aq) → Zn2+ (aq) + Cd(s). (Eºcell = 0.36V) operating at 319.351 K. If (conc. Cd2+) = 0.411 and (conc. Zn2+) = 1.101, calculate the Ecell (volts).
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