AnaleePerezCell Processes and Transport_ Tutorial

Calculate the standard reaction free energy delta G for the following redox reaction. Round to 3 decimal places 4Cl^-(aq)+ N2(g)+4H2O(l)—> 2Cl(g) +N2H4(aq)+ 4OH^- (aq)

The described electrochemical cell (concentration cell) was set up: Cu|CuSO4 (c1) // CuSO4 (c2)|Cu Determine which electrode is the positive terminal (+) of the cell and calculate the cell potential E (electromotive force, EMF) for the given concentrations of the electrolyte CuSO4 in the cell (25oC): c1 = 0.01 mol dm-3, c2 = 1×10-4 mol dm-3

The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". standard concentration Peak area (a.u) (ppm) 50 8354 100 16925 150 25218 200 33584 250 42002 A 50 ml wastewater sample was placed in a coulometric cell, added with excess Kl and starch indicator. Electrolysis was carried out at a constant current of 84.6 mA for 386 s to reach the end point of the titration. What is the concentration of H2S in the sample (in ppm)?

Ohttps://www-awa.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-IBcn9hvCfbYq_fi3Zs O ELECTROCHEMISTRY Using the relationship between charge, current and time An electric current of 0.760 A flows for 54.0 seconds. Calculate the amount of electric charge transported. Be sure your answer has the correct unit symbol and the correct number of significant digits. x10

Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg"(1.0 M) || Pb*?(1.0 M) | Pb 1 2.24 Zn | Zn*2(1.0 M) || Pb*2(1.0 M) | Pb 0,63 3 Mg | Mg*(1.0 M) || Zn*²(1.0 M) | Zn The chemical reaction occurring in first galvanic cell is: Mg + Pb+2 → Mg*2 + Pb 20. What is the standard cell potential for galvanic cell 3 depicted in the table above? (A) 2.87 V (B) 1.61 V (C) - 1.61 V (D) - 2,87 V 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. E* = +0.80 V Ag (aq) + e → Ag(s) Cd"(aq) + 2e → Cd(s) E =-0.40 V Identify the anode and give the…

12:09 PM Thu Apr 6 Question 23 of 24 Calculate the cell potential of the concentration cell described by Ag(s)|Ag*(aq, 0.25 M)||Ag* (aq, 2.00 M)|Ag(s) E°Ag = +0.80 V, T = 25.0 °C | v V S 25 3 6 9 1 4 7. 8 +1- Tap here or pull up for additional resources O Submit X C x 100 YOU

The Nernst-Planck equation (shown below) describes the motion of a charged chemical species in a fluid. dC; z,FC; dv J; = - D; dx RT dx' What are the units for the ion flux J, where: zis the valence state of the ion (unitless) C is the concentration (mol/m³) Fis the Faraday constant (Coulomb/mol) Ris the ideal gas constant (kg m²/(s² mol °K)) Tis the temperature (K) dCi/dx is the concentration gradient (mol/m*) dV/dx is the electric potential gradient (V/m) D; is the diffusion coefficient (m²/s) Note that Coulomb is a unit of charge and V is volts where 1 V= 1 Joule/Coulomb)

5. For the cell Cd(Hg)|CdSO4. H2O(s)|H&2SO4(s)|Hg the emf is given as a function of temperature t (°C), by the emprical expression E(V) = 1.01845 – (4.05 x 10)(t-20) – (9.5 x 10-7)(t-20)? Calculate the changes in the thermodynamic properties of free energy, entropy and enthalpy for the cell reaction at 25°C

6D.4 The potential of the cell Pt(s)|H,(g,p®)[HCI(aq,b)|Hg,Cl,(s)|Hg(1) has been measured with high precision with the following results at 25°C: b/(mmolkg") 1.6077 5.0403 3.0769 7.6938 10.9474 E/V 0.600 80 0.568 25 0.543 66 0.522 67 0.505 32 Determine the standard cell potential and the mean activity coefficient of HCI at these molalities. (Make a least-squares fit of the data to the best straight line.)

The Ksp of CuCl is 1.7 × 10-7. Part A Find Ecell for the cell: Cu(s) | CuCl(s) | CI (aq, 0.40 mol L-1) || Cu* (aq, 0.30 mol L-1) | Cu(s) Express your answer to two significant figures and include the appropriate units. ? Ecell = V Submit Previous Answers Request Answer X Incorrect; Try Again

Write the charge balance for a MgSo, and NaNO, solution that contains H*, OH¯, Mg²+, HSO,, So, MGHSO†, MgOH*, Na+, and NO, . left side of charge balance: right side of charge balance: SPECIAL ΔΣΩ λμπ (s) (1) (aq) (g) () [] CLR

rship X Report - Go tActivity.do?locator=assignment-take Ei Grammarly X NGLSync Pc X OWLv2 | Onl X + Q Use the References to access important values if needed for this question. Consider the following cell reaction: Zn(s) + 2 H+(? M)→→Zn²+(1.00 M) + H₂(g)(1.00 atm) If the cell potential at 298 K is 0.555 volts, what is the pH of the hydrogen electrode? pH = Submit Answer Retry Entire Group 6 more group attempts remaining (? 73°F a 10:47 PM 5/27/2022 E Upc

What is the schematic representation of a cell with a saturated calomel electrode as the reference electrode and a silver indicator electrode to measure the p-function of [CrO4²-]? SCE | Ag2CrO4(sat'd), CrO42-(x M)| Ag O SCE || Ag2 CrO4(s), CrO4²-(x M)| Ag SCE ||Ag2 CrO4(sat'd), CrO4²-(x M) | Ag SCE || Ag2CrO4(s), CrO4²-(x M) | Ag

Calculate the standard cell potential for the following electrochemical reaction. Use the values from Table 20.1 (p .909) in the text. Mn2+(aq) + Sn²+(aq) Mn(s) + Snª+(aq) Answer:

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10. Between 0°C and 90°C, the potential of the cell Pt(s) | Hg. 1.00 atm) | HCK(aq, 0.100 m)| AgCl(s) | Ag(s) is described by the equation: E(V)-0.35510-3.422x10 T-3.2347x106 T2+ 6.314*10⁹T¹ where T is the temperature on the Celsius scale. Calculate A,S for the cell reaction at 50.C. a) -29.9 J/mol .°C b) -33.4 J/mol °C c) -25.2 J/mol.°C )-18.6 J/mol.C

The Ksp of CuCl is 1.7 × 10-7. Part A Find Ecell for the cell: Cu(8) | CuCl(s) | CI (aq, 0.40 mol L-1) || Cu* (aq, 0.30 mol L-1) | Cu(s) Express your answer to two significant figures and include the appropriate units. ? Ecell = V

Part A The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s) H2 (g, 1 atm)|H (aq, ? M)||Cu" (aq, 1.0 M)|Cu(s). What is the pH of the solution if Ecell is 375 mV ? Express your answer using two significant figures. ΑΣφ ? pH = Submit Previous Answers Request Answer X Incorrect; Try Again; 7 attempts remaining ( Return to Assignment Provide Feedback