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- 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. (Correction delta H_f (NH_4Cl (s)*2H_2O (s))=1,404 kJ/mol)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.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
- 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!
- 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.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*10-13The 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.)Express the equilibrium constant (Koverall) for the dissolution of Ag2CO3 in acidic solution (as shown below) using one or a combination of these constants: Ksp of Ag2CO3, Kaj and Ka2 of H2CO3, and Kw- Ag2CO3(s) + 2 H30*(aq) = 2 Ag*(aq) + H2CO3(aq) + 2 H2O) O Koverall = (Ksp x Kw)(Ka1 x Ka2)1 O Koverall = (Ksp) (Ka1)1 O Koverall = Ksp x Ka1 x Ka2 O Koverall = (Ksp)(Ka1 x Ke2)-1The 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!