Homework Answers
Add Answer to:
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)
Most questions answered within 3 hours.
-
You plan to save $5,700 per year for the next 10 years. After
the last deposit,...
asked 9 minutes ago -
On January 1, 2019, ABC Corp. borrowed $81,000 by signing an
installment loan. The loan will be...
asked 13 minutes ago -
Enzyme X exhibits maximum activity at pH = 5.25. X shows a sharp
decrease in its...
asked 28 minutes ago -
Postulate a reason for why so many aliphatic amino acids are
essential.
asked 27 minutes ago -
Three samples were taken of 4 different dog food bags and their
weights were recorded:
Sample/Observation...
asked 30 minutes ago -
The Beatles had 27 number one hits; a radio station asks
listeners to send in a...
asked 28 minutes ago -
Help with Java Program Please
Create a simple graph class. The graph class should have the...
asked 29 minutes ago -
Which of the following statements is true regarding the nature
of culture?
A.We are born with...
asked 50 minutes ago -
(a) 2
NO2(g) à 2
NO(g) +
O2(g)
The rate law for this reaction
is 2nd...
asked 53 minutes ago -
Write the overall reaction for the RedOx
reaction (below) when it occurs in an acidic environment....
asked 59 minutes ago -
Two forces are acting on an object. Force 1 on the object is 6.0
N and...
asked 1 hour ago -
You are planning for retirement. You plan to work for 20 years.
Starting a year from...
asked 1 hour ago