A voltaic cell that uses the reaction PdCl₄^2-(aq) + Cd(s) → Pd(s) + 4 Cl^-(aq) + Cd²⁺(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow

Name: Chemistry: The Central Science
Author: Brown
ISBN: 9780134414232

Verified step by step guidance

Identify the oxidation and reduction half-reactions. In this reaction, Cd(s) is oxidized to Cd2+(aq), and PdCl4^2-(aq) is reduced to Pd(s).

Determine the anode and cathode. The anode is where oxidation occurs, so Cd(s) is the anode. The cathode is where reduction occurs, so PdCl4^2-(aq) is the cathode.

Sketch the voltaic cell. Draw two compartments: one for the anode and one for the cathode. Connect them with a salt bridge to allow the flow of ions.

Label the anode and cathode in your sketch. The anode (Cd) should be on the left, and the cathode (Pd) should be on the right.

Indicate the direction of electron flow. Electrons flow from the anode to the cathode through the external circuit. In this case, electrons flow from the Cd electrode to the Pd electrode.

Key Concepts

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

Voltaic Cell Components

A voltaic cell, also known as a galvanic cell, consists of two electrodes: the anode and the cathode, immersed in an electrolyte solution. The anode is where oxidation occurs, releasing electrons, while the cathode is where reduction takes place, accepting electrons. Understanding these components is essential for sketching the cell and labeling its parts correctly.

Standard Cell Potential

The standard cell potential (E°) is a measure of the voltage produced by a voltaic cell under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It indicates the driving force behind the electrochemical reaction, with a positive value suggesting a spontaneous reaction. In this case, the +1.03 V indicates that the reaction is favorable and helps determine the direction of electron flow.

Electron Flow Direction

In a voltaic cell, electrons flow from the anode to the cathode through an external circuit. This flow occurs because the anode is negatively charged (due to oxidation) and the cathode is positively charged (due to reduction). Understanding this flow is crucial for accurately sketching the cell and indicating the movement of electrons during the electrochemical reaction.

Related Practice

Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (c) Fe1s2 + 2 Fe3+1aq2 ¡ 3 Fe2+1aq2

335

views

Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (d) 2 NO3-1aq2 + 8 H+1aq2 + 3 Cu1s2 ¡ 2 NO1g2 + 4 H2O1l2 + 3 Cu2+1aq2

(b) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell.

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow

Key Concepts

Voltaic Cell Components

Standard Cell Potential

Electron Flow Direction

A voltaic cell that uses the reaction PdCl₄^2-(aq) + Cd(s) → Pd(s) + 4 Cl^-(aq) + Cd²⁺(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow