Calculate e values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. Cr*t (ag) + Cl2 (9) = Cr2O,²- (ag) + Cl¯ (ag) а. V b. Cu?+ (ag) + Mg(s) = Mg²+ (aq) + Cu(s)

Calculate e values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. Cr*t (ag) + Cl2 (9) = Cr2O,²- (ag) + Cl¯ (ag) а. V b. Cu?+ (ag) + Mg(s) = Mg²+ (aq) + Cu(s)

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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Use the References to access important values if needed for this question. A standard galvanic cell is constructed in which a Ni2+ | Ni half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The cathode reaction is Ni²+ + 2e¯ -> Ni In the external circuit, electrons flow from the other compartment to the Ni2+ | Ni compartment. The cathode reaction is Ni -> Ni²+ + 2e- O Ni²+ is reduced at the cathode. The anode compartment could be Fe³+ | Fe²+.
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The electrodes in the following electrochemical cell are connected to a voltmeter as shown. The half-cell on the right contains a standard silver-silver chloride electrode (a silver wire coated with AgCl(s), as in questions 5 and 6). AgCl (s) + e → Ag(s) + CI- (1 M) E° = 0.2223 V The half-cell on the left contains a silver electrode immersed in 100.0 mL of 1.00 x 10-³ M AgNO3(aq). A porous plug through which ions can migrate separates the half-cells. What is the voltmeter reading after 10.00 mL of 0.0100 M K₂ CrO has been added to the half-cell on the left and the mixture has been thoroughly stirred? Hint: Ksp of Ag₂ CrO₂ = 1.1 x 10-1² -Ag(s) Voltmeter 1.00 x 10-3 M AgNO3(aq) Ag. AgCl(s)- 1.00 M KCI
Calculate e values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLV2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. Cr+ (ag) + Cl2 (g) = Cr20,2-(ag) + Cl¯ (aq) b. Ni²+ (ag) +Ba(s) = Ba?+ (ag) + Ni(s)
Calculate € values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a. Cr³+ (aq) + Cl₂ (g) ⇒ Cr₂O7²- (aq) + Cl¯ (aq) €° b. Cu²+ (aq) + Ca(s) Ca²+ (aq) + Cu(s) V
3. write a report on the use of zinc as a “sacrificial anode” to minimise the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K Picture of question 2 is also given
2. For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
Caculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
Silver (Ag) is observed to corrode in HCl (1M activity) in aerated condition. 1) Write the anodic and cathodic half reactions. Write ½ reactions as reduction reactions. 2) What are the standard potentials of the ½ reactions Following the previous question, write the overall reaction? 3) What is the overall potential difference?
Calculate e values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLV2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) a. Cr** (ag) + Cl2 (9) == Cr2O,²- (ag) + Cl¯(aq) E = V b. Cu?+ (ag) + Ba(s) Ba²+ (ag) + Cu(s) V
Calculate e° values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLV2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) a. Cr*+ (ag) + Cl2 (g) = Cr2O,²- (ag) + Cl¯ (ag) V b. Cd²+ (ag) + Ba(s) = Ba2+ (aq) + Cd(s) V