1. Determine the Reaction Order for HCl using calculations described in the background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples, so round to the nearest whole number.2. Determine the Reaction Order for Na2S2O3 using calculations described in the Background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples.3. Write the rate law for the reaction between HCl and Na2S2O3.4. Describe sources of error in this experiment? Data Table 1: Varying Concentrations of HCIWell #C1, D112of Drops ofHCIof Drops of 0H₂O# of Drops of 8Na₂S₂O₂Concentration 1.0(M) ofHCI StockSolutionConcentration 0.30(M) ofNa₂S₂O3StockSolutionReactionConcentration(M) of HCIafter Mixing inWellReactionConcentration(M) ofNa₂S₂O3 afterMixing in WellTrial 1ReactionTime (sec)Trial 2ReactionTime (sec)AverageReactionTime (sec)Reaction"Rate" (sec¹)0.600.1223.4630.0326.70.0375Well #C2, D26681.00.300.150.1241.1531.2236.20.0276Well #C3, D34881.00.300.060.1246.1237.1241.60.0240 Data Table 2: Varying Concentrations of Na₂S₂O3Well #C4, D4#of Drops of 8HCI#of Drops of 0H₂O# of Drops of 12Na₂S₂O3Concentration 1.0(M) ofHCI StockSolutionConcentration 0.30(M) ofNa S₂0₂StockSolutionReactionConcentration(M) of HCIafter Mixing inWellReactionConcentration(M) ofNa₂S₂O, afterMixing in WellTrial 1ReactionTime (sec)Trial 2ReactionTime (sec)AverageReactionTime (sec)Reaction"Rate" (sec¹)0.40.2831.1225.2943.80.0228Well #C5,D5861.00.300.40.04553.2457.47820.0122Well #C6, D68841.00.300.40.0289.8684.93129.90.0077

Dear student I can do only first three parts according to bartleby guidelines. Please post other…

1. Determine the Reaction Order for HCl using calculations described in the background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples, so round to the nearest whole number. 2. Determine the Reaction Order for Na2S2O3 using calculations described in the Background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples. 3. Write the rate law for the reaction between HCl and Na2S2O3.

1. Determine the Reaction Order for HCl using calculations described in the background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples, so round to the nearest whole number. 2. Determine the Reaction Order for Na2S2O3 using calculations described in the Background section. Show your work. Note that your answer will probably not be a whole number as it is in the examples. 3. Write the rate law for the reaction between HCl and Na2S2O3.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.26QAP

See similar textbooks

Similar questions

Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?
KNO3 (aq) added to CaC2O4 (Ksp = 1.3 x 10-8) in solution will lead to __________ in solubility of the solid no effect then decrease increase no effect
a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
PS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTA
A STOCK SOLUTION containing 0.1581 g/L K2CrO4 was prepared.In order to make the CALIBRATION STANDARD, 5 ml of the STOCK was transferredinto a 50ml volumetric flask and then diluted with an appropriate solvent.Calculate:(a) The ppm of K2CrO4 in the CALIBRATION STANDARD.(b) The molarity of K2CrO4 in the CALIBRATION STANDARD. (c) Calculate the molar absorptivity of K2CrO4 (at 371.0 nm). Assume that Beer's Law isobeyed over this concentration range.At 371.0 nm, this CALIBRATION STANDARD in a cell of path length 1.00 cm gave a %T of 59.752.
As solution was prepared by dissolving 5.76g of KCl.MgCl2.6H2O (277.85g/mol) in sufficient water to give 2.000L. calculate a. pMg for the solution b. pCl for the solution
Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate) 2 Fe is sought(Analyte), 1Fe2O3 is weighed (Precipitate)
Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate)
The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the osmotic pressure in atm.