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Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…
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Q: A certain metal M forms a soluble sulfate salt MSO4 . Suppose the left half cell of a galvanic cell…
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Q: A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell…
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- Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.In the temperature range 0-90 ºC , the potential difference of the following cell:Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s)changes as follows with the temperature:Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Result: -34388 J/mol, 10.94 J/Kmol, -30.42 KJ/molIn the temperature range 0-90 ºC , the potential difference of the following cell: Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s) changes as follows with the temperature: Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC. Result: -34388 J/mol, 10.94 J/Kmol, -30.42 KJ/mol
- Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the atomic mass of Ag is 107.868 2 (60.000 2), find the value of the Faraday constant and its uncertainty.In the temperature range 0-90 ºC , the potential difference of the following cell: Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s) changes as follows with the temperature: Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Calculate the standard state AG for the following coupled reactions: A> B K'eq= 1.5 X 10S ×+Y= XY K'eq= 1.5 X 10-4 B+x+Y-A+XY AGO= ????
- The standard electrode potentials for Ag | Ag+ (aq) and Ag (s) | Ag2SO4 (s) | SO42- at 298 K are +0.799 V and +0.652 V, respectively. Determine the solubility product constant of Ag2SO4 at this temperature.[1.1 x 10-5] The answer is wirtten in the bracket. Thank you!Given the ff data at 25 C: cathode= AuNO3 anode= Hydrogen (conc. 1.01 M) In the photo attached is the table for ln [concentration of Au] against potential (V) for the electrochemical cells . It shows how the potential changes when concentration of the cathode is changed (ln concentration) 1. Determine E at y- intercept 2. Calculate delta G and Keq Thank you.If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)
- Calculate the standard potential of the cell Hg(l)|HgCI2(aq)||TINO3(aq)|TI(s) at 25 °C. (b) Calculate the cell potential when the molar concentration of the Hg2+ ion is 0.230 mol dm-3 and that of the Tl+ ion is 0. 720 mol dm-3.6) Chromium can be electroplated from aqueous potassium dichromate, with thereduction shown below. If a current of 6.0A and a voltage of 4.5V are used:Cr2O7+(aq) + 14H+(aq) + 12e- -> 2Cr(s)+7H2Oa) How many hours would it take to completely convert215mL of 1.25M K2Cr2O7 to elemental chromium?b) How many kilowatt-hours of electrical energy arerequired to plate 1.00 g of chromium?a) Given the redox reaction equation below: MnO4 - (aq) + Zn (s) → Mn2+ (aq) + Zn2+ (aq) i. Complete and balance the above equation in acidic solution. ii. Calculate the standard potential produced from the above redox reaction. iii. Write the Qc expression for the above reaction