The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. Type the half-cell reaction that takes place at the anode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s). (1), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation. ▸ View Available Hint(s) ΤΗΓΑΣΦ Cr(s)→Cr' (aq) + 3e¯ DA chemical reaction does not occur for this question. Submit Previous Answers Part C The half-cell is a chamber in the voltaic cell where one half-cell is the site of an oxidation reaction and the other half-cell is the site of a reduction reaction. Type the half-cell reaction that takes place at the cathode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s). (1). or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation. View Available Hint(s) ΑΣΦ 4

The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. Type the half-cell reaction that takes place at the anode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s). (1), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation. ▸ View Available Hint(s) ΤΗΓΑΣΦ Cr(s)→Cr' (aq) + 3e¯ DA chemical reaction does not occur for this question. Submit Previous Answers Part C The half-cell is a chamber in the voltaic cell where one half-cell is the site of an oxidation reaction and the other half-cell is the site of a reduction reaction. Type the half-cell reaction that takes place at the cathode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s). (1). or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation. View Available Hint(s) ΑΣΦ 4

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part A A fuel cell differs from a battery because the current is being generated from a reduction-oxidation (redox) reaction in which the reactant is consumed. A classic example of a fuel cell is the phosphoric acid fuel cell (PAFC), which have been used in stationary power generators, buses, and even submarines. Fuel cells require an electrolyte (similar to batteries) to carry electrically charged species between the electrodes, and a PAFC utilizes phosphoric acid (H3PO4) as its electrolyte. The weak acid phosphoric acid has three acidic protons, highlighted in red here: H3PO4. As a weak acid, some of the acid will remain in molecular form when dissolved in water. Write the net ionic equation that depicts the dissociation of the first proton including charges for any ions produced. Express you answer as net ionic equation including phases. • View Available Hint(s)
So Please don't provide the handwriting solution
5. a) What type of voltaic cell is constructed from half cells consisting of the same electrode material and electrolyte solutions, but with different ion concentration? b) What is the standard emf (E°) of this type of cell?
5. A voltaic cell is constructed using the reaction of chromium metal and iron (II) ions. 2 Cr(s) + 3 Fe*(aq) → 2 Cr*(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the . .electrode to the Negative ions move in the salt bridge from the. .electrode. half-cell to the half-cell. The half-reaction at the anode is , ..and that at the cathode is
1. A voltaic cell consists of two half-cells. One of the half-cells contains a platinum electrode surrounded by chromium (III) and dichromate ions. The other half-cell contains a platinum electrode surrounded by bromate ions and liquid bromine. Assume that the cell reaction, which produces a positive voltage, involves both chromium (III) and bromate ions. The cell is at 25°C. Information for the bromate reduction half reaction is as follows: 2BrO, (ag) + 12н"(аq) + 10е- — Brz () + 6H,0 Ed = 1.478 V (a) Write the cell diagram notation (b) Calculate E° for the cell (c) Calculate the voltage of the cell when all ionic species except H+ are 0.1500M and the pH is at -0.301.
Consider a galvanic cell consisting of: Co2++2e−Co2++2e- →→ CoCo -0.44 Al3++3e−Al3++3e- →→ AlAl -1.66 Write the reaction occurring at the anode: Use spaces only before and after a plus sign. For example, the reaction: Fe2++2e−→FeFe2++2e-→Fe would be entered as: Fe^2+ + 2e^- →→ Fe part1. : Write the reaction occurring at the cathode: part2. : Write the reaction for the galvanic cell: part 3. : Calculate the E0cell for the cell.
Sketch the galvanic cell based on the following overall reactions. Calculate ɛ°; show the direction of electron flow and the direction of ion migration through the salt bridge; identify the cathode and anode; and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. Refer to the table above for the standard reduction potential
What is an electrochemical reaction? What are the four main parts of a galvanic/voltaic cell? Give the function of each part. Provide a definition for each of the four types of redox reactions. Indicate the type of redox reaction each redox reaction is in the section above. Single Displacement Combustion Synthesis Decomposition
2.Write half-reaction for the cell's anode. Include the phases of all species in the chemical equation.
Which of the following is false regarding a voltaic/galvanic cell? Oxidation occurs at the anode and reduction at the cathodeThe cell potential is negative.The reaction is spontaneous.The cell can be used to harness useful work such as electrical energy.
. Suppose we construct a pressure cell in which the gas pressures differ in the two half-cells. Suppose such a cell consists of a Cl2(0.010 atm) | Cl-(1 M) half-cell connected to a Cl2(0.50 atm) | Cl-(1 M) half-cell. Determine which halfcell will be the anode, write the overall equation for the reaction, and calculate the cell potential.
A voltaic cell is constructed from the following half-cells: a magnesium electrode in magnesium sulfate solution and a nickel electrode in nickel sulfate solution. The halfreactions are Mg (s) → Mg2+ (aq) + 2e" Ni?* (aq) + 2e → Ni (s) Sketch the cell, labeling the anode and cathode (and the electrode reactions), and show the direction of electron flow and the movement of cation.