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Indicate the direction of the elll (b) (3pts) Give the balanced half-reactions for each s (a)...
Data Sheet1 I. Oxidation-Reduction Reactions A. The Zn-Cu System Copber tuiting black + pieces cam experimental observations: bubblk fed +arnad same B. The A-Cu system experimental observations: les floaking claud C. The Zn-Pb System Il. Electrochemical Cells A. The Zn-Cu Electrochemical Cell B. The Fe-Cu Electrochemical Cell all otage:402 dv cell voltage: Data Sheet 2 I. Oxidation-Reduction Reactions A. The Zn-Cu System oxidation half-equationS フプ reduction half-equation Caiad the net equation st Cuz not prediction of spontaneity; comparison of predicted...
First fill in your half cell and cell reactions. F in standard cell potentials as you calculate them. Oxidation at the Anode: The black (.) lead is attached to the electrode, which is the source of electrons. Write the anode half reaction: Reduction at the Cathode: The red lead (+) is attached to the electrode. Write the cathode half reaction: E degree - V. Overall Cell Reaction (Net Ionic equation): Write the overall cell reaction (balance electrons and add together):...
1. We will be building a Cu2+ and Zn2+ galvanic cell. Write the two half reactions (one as a reduction and one as an oxidation based on forming a spontaneous reaction) and write the combined reaction. (Similar to equations 9.3-9.5 but for our system specifically). (3 pts) 2. In the galvanic cell we are building in class, which is the anode and which is the cathode? pts) Calculate Ecell for our voltaic cell. (Use Table 16.1 in your OpenStax (Atoms...
Given the following two half reactions with their standard reduction potentials: Rh3+(aq) + 3e− → Rh(s) E° = 0.76 V Au+(aq) + e− → Au(s) E° = 1.69 V What is the cell potential (E, in Volts) for a cell at 298.15 K whose anode consists of [Rh3+] = 0.40 M and Rh(s), and whose cathode consists of [Au+] = 0.10 M and Au(s)?
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
In a battery, two solutions are pumped into each half cee. And the two half- 2. reactions take place at two inert electrodes Pt(s). One reaction is based on the reduction of Sn4+ to Sn2+ in solution, and the other reaction is based on the oxidation of Fe+ to Fe3 in solution. a. Write the ha lf-reactions for each half cell, and label with oxidation reaction and reduction reaction. b. Write the line notation for the cell. C. Write the...
5. A galvanic cell is constructed which uses the following half reactions. The initial concentration of each aqueous reactant and product is 0.100 M. H2O2(aq) + 2H"(aq) + 2e 2H2O() CIO-(aq) H2O(l) + 2Cl(aq) + 2OH(aq) a. Write the line notation for the cell. (5 pts) b. Write the net ionic equation for the cell reaction. (5 pts) c. Calculate the initial potential of the cell. (5 pts) Answer: d. Calculate the pH in the anode and cathode compartments after...
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to Sn^2+(aq). (a) Write half-reactions for the cell's anode and cathode. Include the phases of all species in the chemical equation. Anode Cathode (b) Write a balanced cell reaction. Include the phases of all species in the chemical equation.
5. A galvanic cell is constructed which uses the following half reactions. The initial concentration of each aqueous reactant and product is 0.100 M. H2O2(aq) + 2H+ (aq) + 2e = 2H20(0 CIO-(aq) + H20(1) +2e = Cl-(aq) +20H-(aq) a. Write the line notation for the cell. (5 pts) b. Write the net ionic equation for the cell reaction. (5 pts) c. Calculate the initial potential of the cell. (5 pts) Answer: d. Calculate the pH in the anode and...