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- 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-3Calculate the theoretic delta H_sol (m=1) of the following reaction: Mn+Cl-n*mH2O (s) --> Mn+(aq)+nCl-(aq)+mH2O (l) for both CaCl_2*2H_2O & NH_4Cl using the table below. (The convention is that the standard enthalpy of the formation of ions in solution is referenced to 1 molal. (Correction delta H_f (NH_4Cl (s)*2H_2O (s))=1,404 kJ/mol)Calculate the theoretic delta H_sol (m=1) of the following reaction: Mn+Cl-n*mH2O (s) --> Mn+(aq)+nCl-(aq)+mH2O (l) for both CaCl_2*2H_2O & NH_4Cl using the table below. (The convention is that the standard enthalpy of the formation of ions in solution is referenced to 1 molal.)
- Consider the cell Pt|H,(g) HCI(aq)|AgCl(s)JAg, for which the cell reaction is 2 AgCl(s) + H,(g) and a molality of HCI of 0.020 mol kg', Ecell = +0.4658 V. (i) Write the Nernst equation for the cell reaction. (ii) Calculate A,G for the cell reaction. (iii) → 2 Ag(s) + 2 HCI(aq). At 25 °C Assuming that the Debye-Hückel limiting law holds at this concentration, calculate E'(CI, AgCl, Ag).Determine the emf for the cell Ag (s) | AgCl (s) | HCl (a = 1) | Cl2 (1 atm) | Pt given that the standard electrode potential of the Ag (s) | AgCl (s) | Cl- (aq) electrode is 0.2225 V, and that of the Pt | Cl2 (g) | Cl- (aq) is 1.3595 V.[1.137] The answer is written in the bracket. I would like to know how it is obtained. Thank you!A soluion of 10.0 mL of 0.0500 mol/L AgNO3 is titrated with 0.0250 mol/L NaBr in the cell: VKE||onbekende oplossing||Ag(s) Calculate the potential of the cell after adding 0.1 mL, 10.0 mL, 20.0 mL and 30.0 ml of titrant. E\deg (Ag+, Ag = 0.799 V; E(VKE = 0.244 V; Ksp(ABr) = 5.0*10-13
- AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.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)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 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!5. Erina observed that the borax she uses to clean the house is only partially soluble with water. She found on the internet that borax is composed of sodium tetraborate (Na,B,0;(OH), • 8H,0) and wanted to analyze its solubility. The dissolution of borax is: Na,B,0;(OH), • 8H20(9 = 2 Na (aq) + B40;(OH), (aq) + 8 H20o A 50.0 mL saturated solution was prepared for the experiment. After filtering the solution, a 5.00 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.4320 M HCI. The endpoint was reached after the addition of 4.73 mL titrant. Since the tetraborate anion (B,0;(OH),?) is a weak base, the tetraborate ion reacts with HCI by the reaction: B,0,(OH), (aq) + 2 H*(aq) + 3 H,0g = 4 H;BO3(aq) a. Write the K, expression for the dissolution process.At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 16.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.041 b)0.869 c)0.083 d)0.165 e)0.340
