The answer is given as follows
6. Calculate the actual cell potential for: Ni | Ni (0.0825 M) || Ag(S20,)2 (0.00963 M),...
2. Consider the voltaic cell illustrated below, constructed by coupling a Ni/Ni half-cell with an Ag/Ag* half-cell and allowing them to react spontaneously. Refer to the table of reduction potentials and write the half-reaction that occurs at each electrode (nickel and silver). Then combine the half-reactions into the overall reaction. a. Calculate the standard cell potential. b. Annotate the diagram below. First, randomly label one electrode as Ag and one as Ni. Then identify which is the anode and which...
need help figuring out 12 and 13, all of the questions Cher 103A Electrochemistry -- which of the two diagrams below represents the galvanic cell? The electrolytic cell? How can you tell? Voltmeter Power supply Molten MX D a. For the galvanic cell if the cathode is on the left and the anode is on the right, which direction do the electrons flow? b. For the electrolytic cell in problem 4, where is the cathode, on the left or the...
Given the following information: Ni2+ + 2e- Ni(s) Eº = -0.25 V Ag* + e. Ag(s) E° = 0.80 V 1) Determine the cell potential of the spontaneous redox reaction. 2) Give the net ionic equation for the overall balanced redox reaction. 3) Label the Galvanic Cell below to model the reaction above. Please include: • substances in each compartment • the salt bridge • the anode • the cathode 4) Give the line notation representation of this galvanic cell....
Question 2 Consider a galvanic cell with the following cell notation: Cu(s)|Cu2+(0.0200 M) || Ag+ (0.0200 M)|Ag(s) a) Calculate the electrode potential at the cathode (Ecathode) b) Calculate the electrode potential at the anode (Eanode) c) Calculate the cell potential (Ecell)
B1. Construction of Galvanic Cells a. For each galvanic cells you construct, calculate the theoretical cell potential using the table of the Standard Electrode Potentials from the Chemistry 0130 data booklet. (3 marks) Measured Galvanic Cells Cathode reaction Anode reaction Voltage (V) Cu?*/Cu and Zn/Zn? 0.937 v Zn/Zn2+ and Ag /Ag 1.329v Ag"/Ag and Cu/Cu2+ 0.394v Electrochemistry 9 b. For each galvanic cells, write the overall cell reaction (balanced net ionic equation). • identify the oxidizing agent (OA) and reducing...
pls do all Page 12 of 14 36. (15 points) A spontaneous galvanic cell consists of one half-cell that e ontains Agia) and rea ad one half-cell that contains Cucs) and Cu2+(ag). The standard reduction reactions are listed below Cu2+(aq) + 2 e-→ Cu(s) +0.34 V Identify which half reaction is happening at the anode and the cathode reaction for this spontaneous galvanic cell. a. and write the gwerall Calculate E°cell for this reaction. b. for this reaction. Calculate Δ...
Questions Galvanic Cell Metal and Solution in Cathode Half-cell Cell Potential(v) Metal and Solution in Anode Half-cell Black Wire (-) Red Wire (+) -2.370 Pt/H2 and Nitric Acid Mg and Magnesium Nitrate #1 -0.143 Pt/ H2 and Nitric Acid Pb and Lead (II) Nitrate #2 -0.249 Pt/ H2 and Nitric Acid #3 Ni and Nickel (II) Nitrate 다 5. Based on your information above write the half reactions occurring in each half-cell. Ensure you are writing the correct oxidation or...
Calculate the standard cell potential (∆Eo) for the galvanic cell: Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...
6. Several cell voltages are given in the following table. The standard reduction potential for the Ag/Ag+ pair is: Ag+ + e → Ag(s) Ered=0.800 V (a) Calculate the standard reduction potentials for the other two half-cells (Z/Z3+ and X/X3+.) (6) Fill in the blanks in the table. Write "non-spontaneous" in the appropriate cells. (C) For the remaining pair, write the spontaneous reactions that occur at the cathode and the anode and the balanced overall spontaneous reaction. NOTE: Your answers...