Project 2: Kinetics of Aluminum CorrosionExperiment 4 - Determining the molar absorptivity of copper(II) chloride2.50 x 1030.1330.2254.20 x 1036.00 x 1037.50 x 1031.20 x 1020.3420.4670.7507.Which of the following statements describe R? and its significance in aBeer's Law calibration Plot?a. R2 describes the molar absorptivity for a Beer's Law Calibration plot. R2should equal a number greater than O since absorbance must be apositive number.b. R? describes the path length in beer's law. For a Beer's Law Calibrationplot R? should equal to 1 since the length of the cuvette is 1.0 cm.c. R? describes the goodness of fit for a linear plot. For a Beer's LawCalibration plot, R2 should equal to 1 since the concentration of a solutionis directly proportional to the absorbance of the solution.d. R describes the slope for a Beer's Law Calibration plot. R should equal anumber greater than 0 but less than 1 since the slope is equivalent to1/concentration in the plot.11/ 11

Beer᾿s Law : Decrease in intensity with thickness is directly proportional to concentration.…

Answered: 7. Beer's Law calibration Plot? Which…

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter1: Introduction To Chemistry

Section: Chapter Questions

Problem 1.77PAE

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+ Moore 5e_Ch11 SP2020.pptx: SP X * OWLV2 | Online teaching and lea X oping Cart | The UAB Blazer x VtakeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topica) [References) Use the References to access important values if needed for this question. In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + % I(g) the following data were obtained: HI), M 0.401 0.201 0.101 5.05x102 seconds 519 779 910 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.401 M is s and when the starting concentration is 0.201 M is req (2) 2req The average rate of disappearance of HI from t=0 s to t= 519 s is Ms! (3) The average rate of disappearance of HI from t = 519 s to t= 779 s is Ms! (4) Based on these data, the rate constant for this v order reaction is Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning | Cengage Technical Support Tch 55 F7…
For 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.
The temperature-dependent form of the extended Debye-Hückel equation is (-1.825 × 10°) (eT)¯ 2 Va log (y) = 1+ 2.00/eT where y is the activity coefficient, e is the dielectric constant of water (a unitless quantity), T is the temperature (in Kevin), z is the charge of the ion, µ is the ionic strength (in moles per liter), and a is the ion size parameter (in picometers). The temperature- dependence of the dielectric constant is given by the equation e = 79.755e(-4.6×10~³)(T–293.15) where the temperature is in Kelvin. What is the value of the activity coefficient of Pb2+ at 70.00 °C when the ionic strength is 0.014 M? étv O, hulu MacBook Pro G Search or type URL 24 4. % & 5 8 R. T. Y U F G H K V. M 0O
The Ksp values of silver chromate Ag2Cro4 and silver iodate Ag(IO3) are given below. Ag2Cro4 Ag(IO3) 1.12 x 1012 3.17 x 10°8 Ksp Based on these Ksp values, which of the following is true? In the solution consisting of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42", Ag2Cro4 precipitate will form. In the solution consisting of 1.0 x10-4 MAg* and 1.0 x10-4 M I03", Ag(IO3) precipitate will form. In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3). In the solution consisting of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate first if we add Ag* ions gradually into the above mixture.
The adsorption equilibrium isotherm for aqueous phenol solution and activated carbon can be determined from the following data: c kg phenol/m3 solution q kg phenol/kg carbon 0.3220 0.150 0.1170 0.122 0.0390 0.094 0.0061 0.059 0.0011 0.045 Determine the appropriate isotherm for this experimental run
In a Power-time thermogram of an isothermal titration calorimeter, the power spikes/peaks associated with the sample injections in the sample cell when integrated with respect to time are representative of what? O A. The internal energy of the reaction in the sample cell B. The work done by the reaction in the sample cell O C. The enthalpy of the reaction in the sample cell O D. The total heat capacity of the reaction in the sample cell O E. The molar heat capacity of the sample injected
Part D Let that Za(OH) () is pely insoluble, which signs that the precipitation reaction with NaOH(aq) (pred in the transition) would go to completion Za (aq) + 2NaOH(aq) Zn(OH), () +2Na (₂) you had a 50 L son containing 200 M of Za" (aq) and you wished to add enough 1.30 M NaOH(aq) to precipitate at of the metal, what is the minimum amount of the NaOH(aq) solution you would As that the NaOH(o) son is the only ace of OEE (n) for the precipitation Capress the volume to three significant figures and include the appropriate View Av Haljuj ml. 7
Calculate the Ksp for Ni(OH)2 Ni(OH)2(s) + 2 e- ⟶ Ni(s) + 2OH-(aq); Eo = -0.720 VNi2+(aq) + 2 e- ⟶ Ni(s); Eo = -0.250 V 7.56x1015 1.15x10-8 1.70x10-33 1.32x10-16
The resistances of a series of aqueous NaCl solutions, formed by successive dilution of a sample, were measured in a cell with cell constant (the constant C in the relation K = C/R) equal to 0.2063 cm-1 and the following values were found at 25°C: c/(mol | 0.00050 0.0010 0.0050 0.010 0.020 | 0.050 dm-3) R/W 3314 1669 342.1 174.1 89.08 37.14 Find the molar conductance of Nacl at 25°C at infinite dilution from the graph.
maWhat mass of nickel (in gm) could be formed in a solution of nickel (II) chloride by passing 0.25 amperes for 10 hours. (At.wt. Ni= 58.7, Cl= 35.5 ) ? NICI + 2e Ni + 2CI
Unless noted, be sure to indicate how many significant figures your answer should be reported to. The use of any calculator except your brain or fingers and toes is not permitted. 1. Sodium dichromate reacts with copper in acidic solution as follows (MW's are under each): Na2Cr207 + 3 Cu + 14 HCI 2 CrCl3 + 3 CuCl2 + 7 H2O 221.98 63.55 36.46 158.33 134.45 18.02 Part A) The reaction of 525 mL of 0.450 M HCI in the presence of excess copper and excess sodium dichromate can produce how many grams of copper (II) chloride? Part B) The reaction 50.00 mL of 0.1234 M HCI in the presence of excess sodium chromate and Cu produced 2.3 g of chromium (III) chloride. Calculate the % yield for the reaction.
Fe3+(aq) + SCN (aq) Fe(SCN)2*(aq) How was the equilibrium concentration of Fe(SCN)2+(aq) measured for the purpose of determining the equilibrium constant K? A. By ensuring that SCN- was not in excess relative to Fe3+(aq). B. By measuring the absorbance of the equilibrium samples and using the Beer-Lambert law to determine [Fe(SCN)2+]equ- C. By plotting the absorbance of Fe(SCN)2+(aq) versus concentration and determining the slope. D. By writing the equilibrium constant equation and solving it for [Fe(SCN)2+]equ- E. [Fe(SCN)2+]egu was taken to be equal to the initial concentration of SCN. Jequ

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