Just block 2. Here are the options ### Electrochemical Cell Analysis#### Diagram Description:The image shows an electrochemical cell setup consisting of two half-cells connected by a salt bridge and a voltmeter. - **Left Half-Cell:** - Contains a magnesium (Mg) electrode submerged in a solution labeled $ \text{Mg(NO}_3)_2 $.- **Right Half-Cell:** - Contains a silver (Ag) electrode submerged in a solution labeled $ \text{AgNO}_3 $.- **Connections:** - A voltmeter is connected with leads to each electrode to measure the voltage across the electrodes. - A salt bridge links the two solutions, allowing ions to migrate and maintain electrical neutrality.#### Questions and Prompts:1. **Electrode Reactions and Electron Flow**: - Given the electrochemical cell, select the correct direction for electron flow: - From the Ag electrode to the Mg electrode through the wire - From the Mg electrode to the Ag electrode through the wire - From the Ag electrode to the Mg electrode through the salt bridge - From the Mg electrode to the Ag electrode through the salt bridge2. **Standard Gibbs' Free Energy Change**: - The change in standard Gibbs’ Energy, $ \Delta G $, for the overall reaction is provided as 609 kJ/mol.3. **Resistor Scenario**: - If the voltmeter is replaced with a resistor (allowing current to flow) and the current is maintained at a constant 1.250 A, calculate the time required for...4. **Concentration Change Effect**: - If the concentrations are adjusted to [Mg$^{2+}$] = 5.00 M and [Ag$^{+}$] = 0.0100 M, choose the expected change in cell potential.This educational resource aids in understanding the basic principles of electrochemical cells, electron flow, Gibbs free energy, and concentration effects on cell potential. ### Educational Resource: Electrochemical Cells#### Diagram Description:The image shows a diagram of an electrochemical cell consisting of two electrodes submerged in solutions containing ions. - **Electrodes**: - Magnesium (Mg) electrode is on the left. - Silver (Ag) electrode is on the right.- **Solutions**: - The left compartment contains $ \text{Mg(NO}_3\text{)}_2 $ solution. - The right compartment contains $ \text{AgNO}_3 $ solution.- **Connections**: - A voltmeter is connected to both electrodes to measure the cell potential. - A salt bridge connects the two compartments, allowing ion flow to maintain electrical neutrality.#### Questions and Data:- **Number of Electrons Transferred**: In the balanced cell reaction, the number of electrons transferred is 2.- **Direction of Electron Flow**: Electrons flow from the Mg electrode to the Ag electrode.- **Standard Cell Potential**: The standard cell potential, assuming 1 M concentrations, is +3.16 V.- **Change in Standard Gibbs' Energy ($ \Delta G $)**: For the overall reaction, the change in standard Gibbs' energy is 609 kJ/mol.- **Current Measurement with Resistor**: If the voltmeter is replaced with a resistor allowing current to flow, and the current measures a constant 1.250 A, calculations can be made based on this data.- **Effect of Concentration Changes**: If the concentrations are changed to $[\text{Mg}^{2+}] = 5.00 \, \text{M}$ and $[\text{Ag}^+] = 0.0100 \, \text{M}$, the cell potential would then need to be calculated based on these new conditions. This information provides insights into the operation and characteristics of electrochemical cells, important for understanding principles in electrochemistry and its applications.

Reduction: gain of electron.. At cathode reduction happen and Ag is deposited... Oxidation: loss of…

Question 1 In the balanced cell reac Mg Mg(NO₂), The standard (assuming Voltmeter Given the electrochemical cell in the picture: V salt bridge The silver electrode gains mass be Ag ([Select] from the Ag electrode to the Mg electrode through the wire The electrons would flow from the Mg electrode to the Ag electrode through the wire from the Ag electrode to the Mg electrode through the salt bridge from the Mg electrode to the Ag electrode through the salt bridge AgNO, The change in standard Gibbs' Energy, AG, for the overall reaction would be 609 kJ/mol If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] -0.0100 M, the cell potential would then be [Select]

Question 1 In the balanced cell reac Mg Mg(NO₂), The standard (assuming Voltmeter Given the electrochemical cell in the picture: V salt bridge The silver electrode gains mass be Ag ([Select] from the Ag electrode to the Mg electrode through the wire The electrons would flow from the Mg electrode to the Ag electrode through the wire from the Ag electrode to the Mg electrode through the salt bridge from the Mg electrode to the Ag electrode through the salt bridge AgNO, The change in standard Gibbs' Energy, AG, for the overall reaction would be 609 kJ/mol If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] -0.0100 M, the cell potential would then be [Select]

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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