Indicate whether each statement is true or false: (a) The cathode is the electrode at which oxidation takes place. (b) A galvanic cell is another name for a voltaic cell. (c) Electrons flow spontaneously from anode to cathode in a voltaic cell.

Verified step by step guidance

Step 1: Understand the role of the cathode and anode in electrochemical cells. The cathode is where reduction occurs, and the anode is where oxidation occurs. Therefore, statement (a) is false.

Step 2: Recognize that a galvanic cell and a voltaic cell are two terms for the same type of electrochemical cell, which generates electrical energy from spontaneous redox reactions. Thus, statement (b) is true.

Step 3: Recall that in a voltaic cell, electrons flow spontaneously from the anode, where oxidation occurs, to the cathode, where reduction occurs. Therefore, statement (c) is true.

Step 4: Review the definitions: Oxidation is the loss of electrons, and reduction is the gain of electrons. This helps confirm the roles of the anode and cathode.

Step 5: Summarize the findings: (a) False, (b) True, (c) True, based on the principles of electrochemistry and the definitions of galvanic/voltaic cells.

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 or vice versa. They consist of two electrodes: the anode, where oxidation occurs, and the cathode, where reduction takes place. Understanding the roles of these electrodes is crucial for analyzing the flow of electrons and the overall reaction in the cell.

Galvanic (Voltaic) Cells

A galvanic cell, also known as a voltaic cell, is a type of electrochemical cell that generates electrical energy from spontaneous chemical reactions. In these cells, the anode is negatively charged and the cathode is positively charged, allowing for the spontaneous flow of electrons from the anode to the cathode, which is essential for producing electric current.

Oxidation and Reduction

Oxidation and reduction are complementary chemical processes that involve the transfer of electrons. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. In electrochemical cells, identifying which species is oxidized and which is reduced is vital for understanding the direction of electron flow and the overall cell operation.

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Oxidation and Reduction Reactions

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Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents: MnO₄^-(aq) + Br^-(aq) → MnO₂(s) + BrO₃^-(aq) (basic solution)

Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H₂O₂, have an atypical oxidation state.) (a) NO₂^-(aq) + Cr₂O₇^2-(aq) → Cr³⁺(aq) + NO₃^-(aq) (acidic solution) (b) S(s) + HNO₃(aq) → H₂SO₃(aq) + N₂O(g) (acidic solution) (c) Cr₂O₇^2- (aq) + CH₃OH(aq) → HCOOH(aq) + Cr³⁺(aq) (acidic solution) (d) BrO₃^-(aq) + N₂H₄(g) → Br^-(aq) + N₂(g) (acidic solution)

Textbook Question

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.) H2O21aq2 + ClO21aq2 ¡ ClO2-1aq2 + O21g2 (basic solution)

Textbook Question

Indicate whether each statement is true or false: (c) A salt bridge or permeable barrier is necessary to allow a voltaic cell to operate.

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Textbook Question

A voltaic cell similar to that shown in Figure 20.5 is constructed. One electrode half-cell consists of a silver strip placed in a solution of AgNO3, and the other has an iron strip placed in a solution of FeCl2. The overall cell reaction is Fe1s2 + 2 Ag+1aq2 ¡ Fe2+1aq2 + 2 Ag1s2 (f) In which directions do the cations and anions migrate through the solution?