The following diagram will be used for questions 4-10. You might want to make a sketch of it. A voltaic cell is constructed using Zinc metal and silver metal electrodes . Solutions of silver nitrate and zinc nitrate also were used. From appendix 6 in your text the following reduction potentials (E are listed. Ag (aq) + 1 e --> Ag (s) 0.800 V Zn 2+ + 2 e- --> Zn (s) -0.762V Match the letters on the diagram to the correct substance. Zinc What is the voltage of the above cell at standard conditions? (E (cell) ) (Answer to 3 decimal places) Answer: What is the standard free energy (A G) for the above cell. (Answer in kj to 3 sig figs) Answer: The values for the equilibrium constant (K) for spontaneous reaction like the one above tend to be very large. Calculate the value of K for the reaction above and enter the exponent of 10 that the number has when written in scientific notation. ( For eample if K = 1.23x 10 45 you would enter 45) Answer:

The following diagram will be used for questions 4-10. You might want to make a sketch of it. A voltaic cell is constructed using Zinc metal and silver metal electrodes . Solutions of silver nitrate and zinc nitrate also were used. From appendix 6 in your text the following reduction potentials (E are listed. Ag (aq) + 1 e --> Ag (s) 0.800 V Zn 2+ + 2 e- --> Zn (s) -0.762V Match the letters on the diagram to the correct substance. Zinc What is the voltage of the above cell at standard conditions? (E (cell) ) (Answer to 3 decimal places) Answer: What is the standard free energy (A G) for the above cell. (Answer in kj to 3 sig figs) Answer: The values for the equilibrium constant (K) for spontaneous reaction like the one above tend to be very large. Calculate the value of K for the reaction above and enter the exponent of 10 that the number has when written in scientific notation. ( For eample if K = 1.23x 10 45 you would enter 45) Answer:

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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For each redox reaction, write the half-reactions and draw the cell diagram for a galvanic cell (use short hand cell notation) in which the overall reaction occurs spontaneously. Identify each electrode as either positive or negative. a. Ag(s) + Fe3+ (aq) → Ag+ (aq) + Fe2+ (aq)
Show your solution. Express your answers in appropriate number of significant figures.
Designing a galvanic cell from tw... A chemist designs a galvanic cell that uses these two half-reactions: standard reduction |MnO4(aq)+2H₂O(l)+3e¯ → MnO₂(S)+4OH(aq) Cl₂(g) +2e 2 Cl(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that 0 happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 0 half-reaction O Yes O No ☐v - potential Ered = +0.59 V = +1.359 V ロ→ロ X x10 S
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: Cr(s) + 3 Ag*(aq) → Cr³*(aq) + 3 Ag(s) Which of the multiple choices correctly describes how the cell emf changes when a change is made to the cell? Ca) Adding water to the anode compartment makes the cell emf less positive. C b) Increasing the size of the silver electrode makes the cell emf stay the same. C C) Adding a solution of 1.0 M AGNO, to the cathode compartment makes the cell emf more negative. C d) Adding Na,s to the anode compartment to precipitate chromium sulfide makes the cell emf less positive. Ce) Adding a solution of 5 M Ag* to the cathode compartment makes the cell emf stay the same.
Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…
5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10
PART 2: Answer what is asked for each problem and show your solution. Round your answers to four decimal places and they must be enclosed all in a box. 1. Given the following reduction potentials: Ag*(aq) + e → Ag(s) Zn?"(aq) + 2e → Zn(s) Calculate the cell potential for the following reaction and predict whether the reaction will take place. If it will take place write the cell notation. Znº"(aq) + 2Ag(s)→ Zn(s) + 2Ag*(aq) E° = 0.80 V; E° = -0.76 V 2. A chromium metal was deposited coming from a solution of Cr*³. The amount of the said metal deposited weighs 2.19 g. The process is made possible through a current of 35.2 Amperes in electrolyte cell. Determine the following: a. How much charge (in C) is required? b. How long (in min) would it take for the reaction to occur?
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O
Please don't provide handwritten solution .....
What will be the products of the electrolysis of an 1-M aqueous aluminum chloride (AICI3) solution at 25 °C? (The electrodes themselves are platinum.) (Use the standard electrode potentials table in your online textbook's Appendix to help you answer the question.) No products will be produced. H₂(8) +20H (aq) + Cl₂(g) 4Al(s) + 30₂(g) + 12H*(aq) O 2H₂(g) + 4H₂O(l) + O₂(g) O2Al(s) + 3Cl2(g)