### Question 4**Diagram Description:**The diagram illustrates a concentration cell setup using magnesium electrodes. It consists of two beakers, each containing a magnesium electrode (Mg). The left beaker contains a solution of 0.00100 M Mg(NO₃)₂, and the right beaker contains a solution of 2.50 M Mg(NO₃)₂. A salt bridge connects the two solutions. A voltmeter is connected between the two electrodes to measure the potential difference.**Text Below the Diagram:**- Given the concentration cell pictured above: - The side with the lower concentration is the \[ \text{Select from: } \text{cathode, there is no cathode because the electrodes are the same, anode, catanode} \] - The cell potential would be \[ \text{Select} \] This setup is an example of a galvanic cell where the driving force for electron flow is the concentration gradient between the two solutions. ### Concentration Cell Diagram ExplanationThe image illustrates a concentration cell setup with magnesium electrodes and solutions of magnesium nitrate (\( \text{Mg(NO}_3\text{)}_2 \)) at different concentrations. - **Components of the Cell:** - Two half-cells connected by a salt bridge. - Each half-cell contains a magnesium electrode (Mg). - The left half-cell contains 0.00100 M \( \text{Mg(NO}_3\text{)}_2 \) solution. - The right half-cell contains 2.50 M \( \text{Mg(NO}_3\text{)}_2 \) solution. - A voltmeter is connected across the two electrodes to measure the potential difference.- **Function of the Salt Bridge:** - The salt bridge maintains electrical neutrality by allowing ions to flow between the half-cells.### Questions- Given the concentration cell pictured above, you are required to determine: - **The side with the lower concentration:** Select whether it's the left or right side. - **The cell potential:** A dropdown menu is provided to select the potential, which is influenced by the concentration difference between the two half-cells.This setup is typically used to study the behavior of concentration cells and to calculate the cell potential using the Nernst Equation.

Answer:- This question is answered by using the simple concept of electrochemistry involving the…

Question 4 Mg Voltmeter salt bridge 0.00100 M Mg(NO3)₂ Mg The cell potential would be [Select] 2.50 M Mg(NO₂)₂ Given the concentration cell pictured above: The side with the lower concentration is the ✓ [Select] cathode there is no cathode because the electrodes are the same anode catanode

Question 4 Mg Voltmeter salt bridge 0.00100 M Mg(NO3)₂ Mg The cell potential would be [Select] 2.50 M Mg(NO₂)₂ Given the concentration cell pictured above: The side with the lower concentration is the ✓ [Select] cathode there is no cathode because the electrodes are the same anode catanode

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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