2 3 11. Identify each of the reactions below as synthesis (S), decomposition (D), single replacement (SR), or double replacement (DR). K,O (s) + H,O (1) 2M9CI, (aq) + Na,CO, (aq) 2AI,0, (s) Cu(NO,), (aq) + Zn (s) H,SO, (aq) + 2NAOH (aq) Na,So, (aq) + 2H,0 (I0) 2K (s) + 2H,0 (1) → 2KOH (aq) + H, (g) 20, (g) + N, (9) 2NAF (s) 2KOH (aq) 2NaCI (aq) + M9CO, (s) - 4AI (s) + 3O, (g) Cu (s) + Zn(NO,), (aq) → N,O, (g) - 2Na (s) + F, (g)
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- What is the Importance of kinetics and chemical equilibria in the development of point of care technologies? Please provide at least 2 insights. You may use this as reference: https://knowledge.electrochem.org/encycl/art-g01-glucose.htmFor the reduction 2FeCl3 + SnCl2 =====➔ 2 FeCl2 + SnCl4 in aqueous solution the following data were obtained at 25oC t(min) 1 3 7 11 40 Y 0.01434 0.02664 0.03612 0.04102 0.05058 Where y is the amount of FeCl3 reacted in moles per liter. The initial concentrations of SnCl3 and FeCl3 were respectively, 0.03125, 0.0625 moles/L. a.)Show that the reaction is third order (derive the rate law), and b.) calculate the average specific rate constant.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
- 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.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)].
- What are the dissociation reaction, including phases, of AICI3?If all other variables were kept constant, determine theeffect that the following errors would have on the calculatedpercent yield of the product. Would the yield be expected toincrease, decrease, or would there be no effect? Explainyour reasoning.– The product was insufficiently dried before weighing.– Some of the product was lost during the transfer fromthe Buchner funnel to the evaporating dish.– 7.5 mL of FeCl3 was added instead of 3.0 mL asoutlined in the procedure.– 4.587g of K2C2O4H2O was used instead of exactly4.000g .– The recrystallization step was skipped and theexperiment went straight to vacuum filtration.What is ΔSsurr for a reaction at 28.6 °C with ΔHsys = 38.9 kJ mol-1 ? Express your answer in J mol-1 K-1 to at least two significant figures.
- The table below shows the time-temperature course during reaction of NaOH sample of 2.02 g with 169 mL of 1M HCl.Plot the data, evaluate ΔT and calculate the reaction enthalpy. time/s t/ oC 0 19.75 15 19.80 30 19.85 45 19.89 60 19.97 75 20.02 90 19.98 105 20.13 120 20.34 135 20.87 150 21.62 165 22.40 180 23.20 200 24.49 220 25.81 240 27.09 260 27.37 280 27.35 300 27.34 320 27.31 340 27.31 360 27.27 380 27.25 400 27.24 Give your calculated enthalpy in kJ·mol-1to 3 significant figuresConsider an urban atmosphere containing 100 ppbv NOx and 100 ppbv O3 with T=298K and P=1 atm. NO + O3 --> NO2 + O2 (1) NO2 + hv --> NO + O3 (in the presence of O2) (2) With k1=2.2x10-12 exp(-1430/T) cm3 molecule-1s-1 and k2=1x10-2 s-1 (ie, at noon). Calculate the steady-state concentration of NO and NO2 at noon based on the above reactions.Which of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)