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Given the electrochemical cell below, answer the following questions. S<H2(g) 00 Ag Agt H+ If the...
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...
Given the following electrochemical cell, calculate the potential for the cell n which the concentration of...
Given the following electrochemical cell, calculate the potential for the cell n which the concentration of Ag* is 0.0415 M, the pH of the H cell is 1.400, and the pressure for H2 is held constant at 1 atm. The temperature is held constant at 55oC. H2(g) Ag Ht Ag
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!
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which...
An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+ concentration is that of a buffer consisting of a weak acid, HA(0.136 M), mixed with its conjugate base, A-(0.142 M). The measured cell voltage is E°cell = 0.196 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = _______ Ka = _______
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)
8) An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|...
8) An electrochemical cell consists of a Pt|H+(aq,1.00 M)|H2(g) cathode connected to a Pt|H+(aq)|H2(g) anode in which the H+concentration is that of a buffer consisting of a weak acid, HA(0.115 M), mixed with its conjugate base, A-(0.192 M). The measured cell voltage is E°cell = 0.168 V at 25 °C, with PH2 = 1.00 atm at both electrodes. Calculate the pH in the buffer solution and the Ka of the weak acid. pH = Ka =
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of...
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0275 M, the pH of the H+ cell is 1.850, and the pressure for H2 is held constant at 1 atm. The temperature is held constant at 55°C.
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.15x104 atm, the F concentration is 1.10M, and the Agt con...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.15x104 atm, the F concentration is 1.10M, and the Agt concentration is 1.48M? F2(g)+2Ag(s)2F(aq)+2Ag (aq) Answer. The cell reaction as written above is spontaneous for the concentrations given: D
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.15x104 atm, the...
3. For the electrochemical cell: Pt(s) | H2(1 atm) | H'(I M)I| C u2(1 M) Cu(s),...
3. For the electrochemical cell: Pt(s) | H2(1 atm) | H'(I M)I| C u2(1 M) Cu(s), which one of the following changes will cause an increase in the cell voltage? A) Lower the H2(g) pressure. B) Increase the size/mass of the copper electrode. C) Lower the H (aq) concentration. D) Decrease the concentration of Cu* ion. E) None of the above. 2+
given this electrochemical cell: Concentration of H+ is unknown, Pressure of H2 is constant at 1...
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
Given the following electrochemical cell, calculate the potential for the cell n which the concentration of Ag* is 0.0415 M, the pH of the H cell is 1.400, and the pressure for H2 is held constant at 1 atm. The temperature is held constant at 55oC. H2(g) Ag Ht Ag
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.15x104 atm, the F concentration is 1.10M, and the Agt concentration is 1.48M? F2(g)+2Ag(s)2F(aq)+2Ag (aq) Answer. The cell reaction as written above is spontaneous for the concentrations given: D
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 3.15x104 atm, the...
3. For the electrochemical cell: Pt(s) | H2(1 atm) | H'(I M)I| C u2(1 M) Cu(s), which one of the following changes will cause an increase in the cell voltage? A) Lower the H2(g) pressure. B) Increase the size/mass of the copper electrode. C) Lower the H (aq) concentration. D) Decrease the concentration of Cu* ion. E) None of the above. 2+
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
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