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- Absorbance at 453 nm 8393939 7 fl. oz./20 ml Beer-Lambert's Law (Spectrophotometry) #1 Fe (aq) + KSCN(s) FESCN "(aq) + K" (aq) 3+ To determine the moles of Fe (aq) in a 100. mL sample of an unknown solution, excess KSCN(s) is added to convert all the Fe (aq) into the dark red species FeSCN"(aq), as represented by the equation above. The absorbance of FESCN"(aq) at different concentrations is shown in the graph below. 2+ 0.50 目0.40 0.30 0.20 01 0. 0. 5 x 10-5 10 x 10-5 Concentration of FESCN2+ (M) If the absorbance of the mixture is 0.20 at 453 nm, haw many moles of Fe (aq) were present in the 100. mL sample? (Assume that any volume change due to adding the KSCN(s) Iis negligible.) 3+, 4x10-4 mol 3 x 104 mol (B) 4x 10-6 mol 3x 10-6 molRoughly how far does an infrared beam penetrate into the sample using an ATR-FTIR spectrometer? Select one: 1 pm 1 μm 1 μΜ 1 nm sbiniesnediytem-WA student generates a calibration curve of absorbance versus concentration of Red Dye #40. The equation of the line (with an R-squared of 0.9976) is y = 36385x + 3.724x10 -5. If they found the absorbance of their unknown dye solution to be 0.6585 AU; what is the concentration?
- A student prepared several solutions of Molecule Bright, each at a different concentration. The absorbance of each solution was measured at 405 nm with a path length of 0.730 cm. The student then plotted the absorbance of each sample vs. its concentration (in mM), and found a best-fit line of y = 3.726x + 0.828. Calculate the molar absorptivity of the Molecule Bright (in M-1 cm-1).8- The fluorescence is mainly resulting from which of the following transitions? (P) n→Ã* (Q) 0→ 0* (R) n→ o* (S) ñ→ ñ* (A) P and S (B) Q and R (C)P only (D) S only ICP21.6 The operator for the square of the total spin of two electrons is Stotal = (S₁ + S₂)² = S² + S² + 2(S1xS2x + S1yS2y + $1$22). Given that iħ S₁α = /B₁ S₁,α = 22²1 2 SxB = ħ 2 α, B, S₂α = = 九↓2 ħ α, iħ ħ S,ß α₁ S₂B = 1/- B₁ a, 2 2 show that a (1) a (2) and ß (1) ß (2) are eigenfunctions of the operator Stotal. What is the eigenvalue in each case?
- Why is it most accurate to measure absorbances in the range A = 0.3 to 2?2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?Hooke's Law and Spectroscopy
- 13C(1h) what is bracket mean in this case? is that mean carbon nmr proton nmr in same time?Calculate the energy difference between 589.0 nm and 589.6 nm Group of answer choices 3.43 EE-22 J 3.00 EE-3 J 5.55 EE-20 J none of theseYou have a specimen composed of germanium and iron, distributed uniformly. The XRF spectrum shows two Kα Kβ doublets, characteristic for the two elements. The intensity (i.e., line amplitude) of Kα Fe is equal to the intensity of the Kα Ge. Can you conclude that there are equal contents of Fe and Ge in your specimen? Explain.