Ch.20 - Electrochemistry

Problem 53

Chapter 20, Problem 53

Use line notation to represent each electrochemical cell in Problem 43.

Verified step by step guidance

Identify the anode and cathode in the electrochemical cell. The anode is where oxidation occurs (loss of electrons), and the cathode is where reduction occurs (gain of electrons).

Write the half-reactions for both the anode and the cathode. The half-reaction at the anode will show the species losing electrons, and the half-reaction at the cathode will show the species gaining electrons.

Combine the half-reactions using a vertical line '|' to separate different phases or states of matter and a double vertical line '||' to represent the salt bridge or porous barrier that separates the two half-cells.

Ensure the line notation follows the order: anode material | anode ion (concentration if given) || cathode ion (concentration if given) | cathode material.

Check the line notation for consistency and completeness, ensuring it accurately represents the physical setup of the electrochemical cell described in Problem 43.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electrochemical Cells

Electrochemical cells are devices that convert chemical energy into electrical energy through redox reactions. They consist of two electrodes, an anode where oxidation occurs, and a cathode where reduction takes place. Understanding the function and components of these cells is essential for representing them accurately in line notation.

Line Notation

Line notation is a standardized way to represent electrochemical cells, providing a clear and concise format for describing the components and reactions occurring within the cell. It typically includes the anode and cathode separated by a double vertical line, with the phases of the reactants and products indicated. This notation helps in visualizing the flow of electrons and the overall cell reaction.

Oxidation and Reduction

Oxidation and reduction are fundamental concepts in electrochemistry, representing the loss and gain of electrons, respectively. In an electrochemical cell, the anode undergoes oxidation (loses electrons), while the cathode undergoes reduction (gains electrons). Understanding these processes is crucial for correctly identifying the half-reactions and representing them in line notation.

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Oxidation and Reduction Reactions

Related Practice

Textbook Question

Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. Ni²⁺(aq) + Mg(s) → Ni(s) + Mg²⁺(aq)

Calculate the standard cell potential for each of the electro- chemical cells in Problem 43.

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Textbook Question

Consider the voltaic cell:

d. Indicate the direction of anion and cation flow in the salt bridge

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Textbook Question

Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°_cell. Sn(s) | Sn²⁺(aq) || NO(g) | NO₃^–(aq), H⁺(aq) | Pt(s)

Is the question formulating correctly? If yes, return the question without changes. If not, please fix it and return the output as a JSON of the form: {'question': 'question text'}. Here is the question: Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell. Mn(s) | Mn2+(aq) || ClO2-(aq) | ClO2(g) | Pt(s)

Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ni(s) + Zn²⁺(aq) → Ni²⁺(aq) + Zn(s)

b. Ni(s) + Pb²⁺(aq) → Ni²⁺(aq) + Pb(s)

c. Al(s) + 3 Ag⁺(aq) → Al³⁺(aq) + 3 Ag(s)

d. Pb(s) + Mn²⁺(aq) → Pb²⁺(aq) + Mn(s)

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