A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. The reaction is: Zn(s)+2Ag*(aq) Zn2+(aq) + Ag(s) Which statement is true regarding the direction of electron flow through the external wire? Zinc Siver O Electrons flow from left to right, from the Zinc to the Silver O Electrons flow from right to left, to the Zinc to the Silver O The zinc electrode will get larger as more zinc forms. OAnions will flow through the "bridge" from the zinc side to the silver side
A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. The reaction is: Zn(s)+2Ag*(aq) Zn2+(aq) + Ag(s) Which statement is true regarding the direction of electron flow through the external wire? Zinc Siver O Electrons flow from left to right, from the Zinc to the Silver O Electrons flow from right to left, to the Zinc to the Silver O The zinc electrode will get larger as more zinc forms. OAnions will flow through the "bridge" from the zinc side to the silver side
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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![### Understanding Voltaic Cells
A voltaic cell, also known as a galvanic cell, is an electrochemical cell that uses a chemical reaction to generate electrical energy. It consists of two different metals connected by a salt bridge or a porous disk between the individual half-cells.
#### Reaction in the Voltaic Cell
In this example, the voltaic cell is constructed based on the oxidation of zinc metal (Zn) and the reduction of silver cations (Ag⁺). The solutions used are silver nitrate (AgNO₃) and zinc nitrate (Zn(NO₃)₂).
The overall chemical reaction is:
\[ \text{Zn(s)} + 2\text{Ag}^+(\text{aq}) \rightarrow \text{Zn}^{2+}(\text{aq}) + 2\text{Ag(s)} \]
#### Diagram Explanation
The diagram shows two compartments:
1. **Left Compartment (Zinc Half-Cell)**:
- Labeled as "Zinc".
- Contains a zinc metal electrode immersed in a zinc nitrate solution.
- Electrons are released from the zinc electrode as zinc metal is oxidized to zinc ions (\( \text{Zn(s)} \rightarrow \text{Zn}^{2+}(\text{aq}) \)).
2. **Right Compartment (Silver Half-Cell)**:
- Labeled as "Silver".
- Contains a silver electrode immersed in a silver nitrate solution.
- Silver ions gain electrons and are reduced to form silver metal (\( \text{Ag}^+(\text{aq}) \rightarrow \text{Ag(s)} \)).
There is an external wire connecting the zinc electrode to the silver electrode, allowing electrons to flow between the two electrodes. There is also an implied salt bridge or porous barrier (not shown in the diagram) allowing ions to flow between these two solutions to maintain charge balance.
#### Questions and Explanation
The question asks about the true statement regarding the direction of electron flow through the external wire:
- A. Electrons flow from left to right, from the Zinc to the Silver.
- B. Electrons flow from right to left, to the Zinc to the Silver.
- C. The zinc electrode will get larger as more zinc forms.
- D. Anions will flow through the "bridge" from the zinc side to the silver side.
**Correct Answer: A. Electrons flow from left to right](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ec4e4dd-380a-451c-aeb3-9cf66efaad71%2F1bf51659-4f1b-4e06-a766-73231313ec80%2F1bisl2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding Voltaic Cells
A voltaic cell, also known as a galvanic cell, is an electrochemical cell that uses a chemical reaction to generate electrical energy. It consists of two different metals connected by a salt bridge or a porous disk between the individual half-cells.
#### Reaction in the Voltaic Cell
In this example, the voltaic cell is constructed based on the oxidation of zinc metal (Zn) and the reduction of silver cations (Ag⁺). The solutions used are silver nitrate (AgNO₃) and zinc nitrate (Zn(NO₃)₂).
The overall chemical reaction is:
\[ \text{Zn(s)} + 2\text{Ag}^+(\text{aq}) \rightarrow \text{Zn}^{2+}(\text{aq}) + 2\text{Ag(s)} \]
#### Diagram Explanation
The diagram shows two compartments:
1. **Left Compartment (Zinc Half-Cell)**:
- Labeled as "Zinc".
- Contains a zinc metal electrode immersed in a zinc nitrate solution.
- Electrons are released from the zinc electrode as zinc metal is oxidized to zinc ions (\( \text{Zn(s)} \rightarrow \text{Zn}^{2+}(\text{aq}) \)).
2. **Right Compartment (Silver Half-Cell)**:
- Labeled as "Silver".
- Contains a silver electrode immersed in a silver nitrate solution.
- Silver ions gain electrons and are reduced to form silver metal (\( \text{Ag}^+(\text{aq}) \rightarrow \text{Ag(s)} \)).
There is an external wire connecting the zinc electrode to the silver electrode, allowing electrons to flow between the two electrodes. There is also an implied salt bridge or porous barrier (not shown in the diagram) allowing ions to flow between these two solutions to maintain charge balance.
#### Questions and Explanation
The question asks about the true statement regarding the direction of electron flow through the external wire:
- A. Electrons flow from left to right, from the Zinc to the Silver.
- B. Electrons flow from right to left, to the Zinc to the Silver.
- C. The zinc electrode will get larger as more zinc forms.
- D. Anions will flow through the "bridge" from the zinc side to the silver side.
**Correct Answer: A. Electrons flow from left to right
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