### Question 1**Diagram Explanation:**The image shows an electrochemical cell setup. It consists of two half-cells connected by a salt bridge and joined to a voltmeter. The left half-cell has magnesium (Mg) immersed in a solution of magnesium nitrate \((\text{Mg(NO}_3)_2)\), and the right half-cell contains silver (Ag) in a silver nitrate \((\text{AgNO}_3)\) solution.#### Questions:1. **Given the electrochemical cell in the picture:** a. **In the balanced cell reaction, the number of electrons transferred is** [Select] b. **The electrons would flow** [Select] c. **The standard (assuming 1 M concentrations) cell potential is** [Select] d. **The change in standard Gibbs' Energy, \(\Delta G\), for the overall reaction would be** [Select] e. **The [Select]** f. **If the voltmeter is replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take** [Select] g. **If the concentrations were changed to \([\text{Mg}^{2+}] = 5.00 \, \text{M}\) and \([\text{Ag}^+] = 0.0100 \, \text{M}\), the cell potential would then be** [Select]#### Diagram Details:- **Components:** - **Voltmeter:** Measures the potential difference between the two electrodes. - **Salt Bridge:** Maintains electrical neutrality by allowing the movement of ions between the two solutions. - **Electrodes:** Mg on the left, Ag on the right.- **Half-Cell Reactions:** - **Anode (Mg):** Mg(s) → Mg\(^{2+}\)(aq) + 2e\(^{-}\) - **Cathode (Ag):** Ag\(^{+}\)(aq) + e\(^{-}\) → Ag(s)The queries relate to the understanding of electrochemical cell operations and various calculations like determining the cell potential, Gibbs' free energy change, and effects of changes in concentration on the cell's potential. **Question 1**The image shows a diagram of an electrochemical cell with the following components:- **Voltmeter:** Connected to measure the potential difference across the cell.- **Salt Bridge:** Allows the flow of ions to maintain charge balance.- **Electrodes:** Magnesium (Mg) and Silver (Ag).### Electrochemical Cell Description:- **Left Side:** - **Electrode:** Magnesium (Mg) - **Solution:** Magnesium Nitrate (\(\text{Mg(NO}_3\text{)}_2\))- **Right Side:** - **Electrode:** Silver (Ag) - **Solution:** Silver Nitrate (\(\text{AgNO}_3\))### Questions and Options:1. **Given the electrochemical cell in the picture:** - **In the balanced cell reaction, the number of electrons transferred is:** - [Select] - **The electrons would flow:** - [Select] - **The standard (assuming 1 M concentrations) cell potential is:** - [Select] - **The change in standard Gibbs' Energy, \(\Delta G\), for the overall reaction would be:** - [Select]2. **Statements with checkbox options:** - Silver electrode gains mass because the silver is oxidized. - Magnesium electrode gains mass because the magnesium is oxidized. - Magnesium electrode gains mass because the magnesium ions are reduced. - Silver electrode gains mass because the silver ions are reduced.3. **Calculation Questions:** - If a current is measured to be a constant 1.250 A, it would take [Select] time for a specific change. - If the concentrations were changed to \([\text{Mg}^{2+}]=5.00 \text{M and } [\text{Ag}^+]=0.0100 \text{M}\), the cell potential would be: - [Select]**Question 2**[Not shown in the image.]

In a given electrochemical cell, at anode, the oxidation occurs while reduction happens at the…

Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred is [Select] The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential is [Select] The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select] The [Select] 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 [Select] If the concentrations were changed to [Mg] -5.00 M and [Ag] -0.0100 M, the cell potential would then be [Select]

Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred is [Select] The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential is [Select] The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select] The [Select] 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 [Select] If the concentrations were changed to [Mg] -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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A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGO. . • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. cell n A B U 2 2 2 calculated quantities (Check the box next to any that are wrong.) AGⓇ 64, kJ/mol O -160, kJ/mol -228. kJ/mol O O K -12 6.13 X 10 O -29 9.32 × 10 O 1.14 X 10 40 O 0 E 0.33 V 0.83 V 1.18 V O O G o
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