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Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations...
Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2and a silver electrode...
Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2and a silver electrode immersed in 1.0 M Agt. Zn2+ + 2e- → Zn E° = -0.76 V Agt + e- Ag E = 0.80 V Calculate Eº and AGº for this cell Calculate AGº for the reaction: 2 Zn (g) + O2 (g) + 2 H20 (1) ► 2 Zn2+ (aq) + 4 OH (aq) Reduction Half-Reaction E° (V) O2(g) + 2 H20 (1)+4 e-®4 OH(aq) +0.403...
Q. Consider a galvanic cell with a zinc electrode immersed in 1.0M Zn2+ and a silver...
Q. Consider a galvanic cell with a zinc electrode immersed in 1.0M Zn2+ and a silver electrode immersed in 1.0M Ag+. Which of the electrodes is the anode? Zn2 + 2e- --> Zn E° = -0.76 V Ag+ + e- --> Ag E° = 0.80 V
A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution...
A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution and a silver electrode immersed in a 1.0 M Ag+ solution. What is the overall equation for this cell?
1-One-half of an electrochemical cell consists of a pure Zinc electrode in a solution of Zn2+...
1-One-half of an electrochemical cell consists of a pure Zinc electrode in a solution of Zn2+ ions; the other half is a Lead electrode immersed in a solution of Pb2+ solution. The half-cell potentials for Zinc and Lead are -0.763 V and -0.126 V, respectively. (a) If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. (b) Compute the cell potential at 25oC if the Zn2+ and Pb2+ concentrations are 10-2...
an electrochemical cell consists of a silver electrode in contact with 346mL of 0.100 M AgNO3...
an electrochemical cell consists of a silver electrode in contact with 346mL of 0.100 M AgNO3 solution and magnesium electrode wit 288mL of a 0.100 M Mg(NO3)2 solution. (a) What is the emf of the cell? (b) What is the spontaneous cell reaction? (c) a current is drawn from then cell until 1.20g of silver have deposited on the silver electrode. What is the emf for the cell at this stage of the operation? (d) What is the equilibrium constant...
Help! Electrochem questions: (1) An electrochemical cell consisting of a cadmium electrode immersed in a solution...
Help! Electrochem questions: (1) An electrochemical cell consisting of a cadmium electrode immersed in a solution of 0.001M cadmium (II) nitrate, and a hydrogen electrode. The hydrogen electrode contains a solution of hydrogen cyanide. The pressure of the hydrogen gas is 1 atm. What is the concentration of the acid when there is measured a potential of 0,220V at 25 ° C. (2)A galvanic cell is composed of copper / copper ion solution (0.1M) on the one hand, and a...
An electrochemical cell is constructed such that on one side a pure nickel electrode is in...
An electrochemical cell is constructed such that on one side a pure nickel electrode is in contact with a solution containing Ni2+ ions at a concentration of 5*10-3 M. The other cell half consists of a pure Fe electrode that is immersed in a solution of Fe2+ ions having a concentration of 0.3 M. At what temperature will the potential between the two electrodes be +0.140 V?
3. Consider a galvanic cell with a copper electrode immersed in 1.0 M Cu and a...
3. Consider a galvanic cell with a copper electrode immersed in 1.0 M Cu and a silver electrode immersed in 1.0 M Ag Cu +2e-Cu E 0.34 V Ag +e-Ag (1pt) Calculate E° for this cell. a. b. (1pt) Identify the anode and cathode. (1pt) Identify the oxidizing and reducing agent. c.
An electrochemical cell is set up with a lead metal electrode immersed in a 0.1393 M...
An electrochemical cell is set up with a lead metal electrode immersed in a 0.1393 M solution of Pb2+ joined, through a salt bridge, to a 0.0511 M solution of Cd2+ into which is placed a cadmium metal electrode. Calculate the potential of this cell in its galvanic configuration and write out the shorthand notation for the galvanic cell.
Be sure to answer all parts. A galvanic cell consists of a silver electrode in contact...
Be sure to answer all parts. A galvanic cell consists of a silver electrode in contact with 305 mL of 0.100 M AgNO3 solution and a magnesium electrode in contact with 265 mL of 0.700 M Mg(NO3)2 solution. (a) Calculate E for the cell at 25°C. V (b) A current is drawn from the cell until 2.20 g of silver have been deposited at the silver electrode. Calculate E for the cell at this stage of operation. V
Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2and a silver electrode immersed in 1.0 M Agt. Zn2+ + 2e- → Zn E° = -0.76 V Agt + e- Ag E = 0.80 V Calculate Eº and AGº for this cell Calculate AGº for the reaction: 2 Zn (g) + O2 (g) + 2 H20 (1) ► 2 Zn2+ (aq) + 4 OH (aq) Reduction Half-Reaction E° (V) O2(g) + 2 H20 (1)+4 e-®4 OH(aq) +0.403...
3. Consider a galvanic cell with a copper electrode immersed in 1.0 M Cu and a silver electrode immersed in 1.0 M Ag Cu +2e-Cu E 0.34 V Ag +e-Ag (1pt) Calculate E° for this cell. a. b. (1pt) Identify the anode and cathode. (1pt) Identify the oxidizing and reducing agent. c.
Be sure to answer all parts. A galvanic cell consists of a silver electrode in contact with 305 mL of 0.100 M AgNO3 solution and a magnesium electrode in contact with 265 mL of 0.700 M Mg(NO3)2 solution. (a) Calculate E for the cell at 25°C. V (b) A current is drawn from the cell until 2.20 g of silver have been deposited at the silver electrode. Calculate E for the cell at this stage of operation. V
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