What is the value of K. expression for the following reaction? Iz(aq) + 5HsIOg(aq) 5710;"(aq) + 9H2O +7H“(aq) In case of first order type "1".
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What is the value of Kc expression for the following reaction?:
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- Provided the reaction A + 2B + C → 2D + E, and the set of data thatfollows:Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
- For the reaction NH2SO2OH + H2O → NH4HSO4 In aqueous solution at 80.35oC, the following constants were observed at the indicated ionic strength μ x103 k (L/mol hr) 5.06 1.07 11.21 1.02 15.85 0.976 22.94 0.886 From these data ascertain: a.) the valence of the reacting ions and b.) the rate constant for the primary salt effect.The progress of the reaction between Iodine ions and potassium iodate(V) can be followed by withstanding samples of the reaction mixture at various times, quenching and then titrating with standard thiosulphate solution. The reaction equation is: I(aq) + IO3(aq) + 6H+(aq) + 4e ➡ I2(aq) + 3H2O(l) In one such experiment the following data were obtained. (see figure below) Determine the order of the reaction with respect to I(aq) and IO3(aq) ions Write the rate expression for the reaction.The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
- The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.The binding of Mg2+ to glycolate anion, (HO-CH2-COO-) proceeds by thisequilibrium:Mg2+ + HO-CH2-COO- ->Mg2+(HO-CH2-COO-) a) Write the expression for Keq for this reversible reaction. b) If you begin with 5 mM Mg2+ and 0.1 mM HO-CH2-COO-, and with a value of Keq = 103 M-1, calculate the concentrations of Mg2+ , HO-CH2-COO-, and Mg2+(HO-CH2-COO-) at equilibrium.In the adsorption of a certain solute, from an aqueous solution on activated carbon at 21°C, the Freundlich constants are n=2.319 and K=0.702 when the equilibrium concentration c is expressed in mol/L a) If 0.1186 g. of this solute is adsorbed on 0.5017 g. of activated carbon at 21°C, find c b) Find the molar mass of solute adsorbed from 0.05 L of a solution whose initial concentration is 0.120 M.
- Suppose that something had gone wrong in the Big Bang, and instead of ord inary hydrogen there was an abundance of deuterium in the universe . There would be many subtle changes in equilibria, particularly the deuteron transfer equilibria of heavy atoms and bases. The Kw for D2O, heavy water, at 25 °C is 1.35 x 10-15. (a) Write the chemical equation for the autoprotolysis (more precisely, autodeuterolysis) of D2O. (b) Evaluate pKw for D2O at 25 ° C. (c) Calculate the molar concentrations of D3O+ and OD- in neutral heavy water at 25 °C . (d) Evaluate the pD and pOD of neutral heavy water at 25 °C. (e) Formulate the relation between pD, pOD, andpKw(D2O).If the concentration of Sn2+ ions in a solution of Sn(OH)2 was measured to be (1.41x10^-3), what is the Ksp value for Sn(OH)2?Define the terms in. and limit the generality of. the expression In k, = In A- E) RT; w hy might there be deviationsfrom the Arrhenius expression?