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nF 30. The standard cell potential (Ecell) of the reaction below is +0.126 V. The value...
please helpppp!!! 7) The standard cell potential (E cell) f for the reaction below i ls...
please helpppp!!!
7) The standard cell potential (E cell) f for the reaction below i ls -0 43 V. The cell potential for this at best cong (6 polnts) Ag Acid 6 natch the H idding 6e e cancel e, pposite pposite (e) e ancel is the he por Poten 8) The standard cell potential (E-cell) of the reaction below is .0.126 V. The value of ΔG" for the reaction is Pb (o) 2H (aq)Pb2+ (aq) H2 (g) vith (6...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° =...
Pb2+(aq) + 2e− ⇌ Pb(s) E° = -0.126 V 2H+(aq) + 2e− ⇌ H2(g) E° = 0.000 V E°cell (in V)= 0.126 V 2. The electrochemical cell is comprised of a Pb electrode in a 1.67 × 100 M solution of Pb2+ (aq) coupled to a Pt electrode in a solution containing H+ (aq) where the pH of the solution is 0.37 and the partial pressure of H2(g) is 0.571 atm. The temperature of the cell is held constant at...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential below, Cut2 (aq) + 2 e. ----> Cu (s) ° = 0.337 volts Pb+2 (aq) + 2 e--...-> Pb(s) ° = -0.126 volts 0.211 V 0.463 V -0.463 V -0.211 V In Part III, to light up a white LED bulb will require forward voltage (VF) at 20 mA. • 5 1.2. 2.0 Calculate the cell potential difference, Eºcell ( cell = Eºcathode -...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) |...
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
53-54 53) The standard cell potential (E®cell) of the reaction below is -0.55 V. The value...
53-54
53) The standard cell potential (E®cell) of the reaction below is -0.55 V. The value of AGº for the reaction is J/mol. 12 (s) + 2Br- (aq) → 21- (aq) + Br2 (1) A) 0.55 B) 5.5 x 10-6 C) 1.1 x 105 D) 0.54 E) none of the above 54) The standard cell potential (Eºcell) of the reaction below is +1.34 V. The value of AGº for the reaction is kJ/mol 3 Cu (s) + 2 MnO4- (aq)...
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode....
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.13 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Pb2+/Pb couples are 0.00 and -0.13 V, respectively. voltmeter saltbridge 1+ Pl(s) LPH2 (g) O Pb2+(aq) + H2(g) --> Pb(s) + 2H+(aq) O Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g)
When the following redox reaction is carried out in a voltaic cell, the standard cell potential,...
When the following redox reaction is carried out in a voltaic cell, the standard cell potential, E°cell, is 0.93 V. What is ΔG° for this reaction at a temperature of 298.15 K? Pb(s) + 2 Ag+(aq) → Pb2+(aq) + Ag(s) A. -180 kJ B. -90 kJ C. 90 kJ D. 180 kJ
For the cell shown, the measured cell potential, Ecell, is−0.3587 V at 25 °C.Pt(s)...
For the cell shown, the measured cell potential, Ecell, is −0.3587 V at 25 °C.Pt(s) | H2(g,0.849 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, E⁰, are2H+(aq)+2e−⟶H2(g) E⁰=0.00 VCd2+(aq)+2e−⟶Cd(s) E⁰=−0.403 VCalculate the H+ concentration.
please helpppp!!!
7) The standard cell potential (E cell) f for the reaction below i ls -0 43 V. The cell potential for this at best cong (6 polnts) Ag Acid 6 natch the H idding 6e e cancel e, pposite pposite (e) e ancel is the he por Poten 8) The standard cell potential (E-cell) of the reaction below is .0.126 V. The value of ΔG" for the reaction is Pb (o) 2H (aq)Pb2+ (aq) H2 (g) vith (6...
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential below, Cut2 (aq) + 2 e. ----> Cu (s) ° = 0.337 volts Pb+2 (aq) + 2 e--...-> Pb(s) ° = -0.126 volts 0.211 V 0.463 V -0.463 V -0.211 V In Part III, to light up a white LED bulb will require forward voltage (VF) at 20 mA. • 5 1.2. 2.0 Calculate the cell potential difference, Eºcell ( cell = Eºcathode -...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
53-54
53) The standard cell potential (E®cell) of the reaction below is -0.55 V. The value of AGº for the reaction is J/mol. 12 (s) + 2Br- (aq) → 21- (aq) + Br2 (1) A) 0.55 B) 5.5 x 10-6 C) 1.1 x 105 D) 0.54 E) none of the above 54) The standard cell potential (Eºcell) of the reaction below is +1.34 V. The value of AGº for the reaction is kJ/mol 3 Cu (s) + 2 MnO4- (aq)...
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.13 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Pb2+/Pb couples are 0.00 and -0.13 V, respectively. voltmeter saltbridge 1+ Pl(s) LPH2 (g) O Pb2+(aq) + H2(g) --> Pb(s) + 2H+(aq) O Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g)
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