Pt(s) |X (aq). X2+ (aq) || Y3+ (aq) IY(s) Given the line notation: where: x2+ +e - X - ** E° = 0.45 V y3+ + 3 e - Y E° = -2.03 V Pt4+ + 4 e Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign

Pt(s) |X (aq). X2+ (aq) || Y3+ (aq) IY(s) Given the line notation: where: x2+ +e - X - ** E° = 0.45 V y3+ + 3 e - Y E° = -2.03 V Pt4+ + 4 e Pt E° = 1.20 V Calculate the EMF. Input values only with 2 decimal places. Do not include the unit. If positive value: DO NOT include the positive (+) sign If negative value: Please include the negative (-) sign

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 3P

See similar textbooks

Similar questions

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= ????
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)
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/mol
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/mol
1) Since E0 (Fe3 + / Fe2 +) = + 0.77 V, E0 (Fe2 + / Feo) = - 0.44 V and E0 (MnO4- / Mn2 +) = +1.51 VFe / Fe3 + (0.01M) // pH = 3; MnO4- (0.10M); Mn2 + (0.01M) / PtWrite down the anode, cathode and total battery reactions of the battery. Calculate the cell potential at a temperature of 25 degrees Celsius and the equilibrium constant of the spontaneous reaction in the cell with the Gibbs Free Energy Change.
Rose was studying the electric field effect on bacterial growth when he unknowingly carried out an anodic reaction on the platinum electrode that led to the discovery of the anticancer drug cisplatin, cis-[PtCl2(NH3)2]. > Determine the formation constant (Kf) of cisplatin at 25 °C.
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
2V is applied across an electrolytic cell containing 1.0M NaNO3. What reaction occurs at the anode? Show your work What reaction occurs at the cathode? Show your work Diagram the cell (assume the two electrodes are in 1 beaker). How many minutes does it take to form 10.0L of your anodic product measured at 99.8kPa and 28oC if a current of 1.3A is passed through the electrolytic cell?
Consider a hydrogen electrode in H Br(aq) at 25 °C operating at 145 bar. Estimate the change in the electrode potential when the solution is changed from 5.0 mmol dm-3 to 15.0 mmol dm-3.
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.
Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of Cl2 at 650 mmHg pressure and 27 degrees Celsius. Calculate the value of Faraday's constant from these data.
A. Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) Express your answer to three significant figures and include the appropriate units. B. Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘= -569 kJkJ and ΔS= -173 J/KJ/K . Express your answer to three significant figures and include the appropriate units.