Find the [FeSCN^2+]eq ε=4.0×10^3 M-1 cm^-1 at 447 nm

A photon of light has a wavelength of 1967 nm. Calculate the energy for 1 photon of light. h = 6.626 x 10-34 J*s, c = 3.00 x 10° m/s, Na = 6.02 x 1023 %3D 1.525 x 1014, 60,840 J 1.011 x 10-34, 1.011 x 10-19,

A liquid sample was analyzed for Fe³+. A plot of absorbance (y-axis) vs. concentration (ppm; x-axis) of the external standards produced a calibration line with an equation y = 0.2256x -0.0903 (R² = 0.9973). The absorbance of the sample was 1.25. Determine the amount of Fe³+ in the sample (in ppm).

2) In a laboratory study, a calibration was performed using NH4C1 to analyze ammonium spectrophotometrically. The results of the study are given below. According to this, when the 5.0 mL sample containing ammonium is completed to 50 mL with pure water, find the amount of NH4 in the sample whose absorbance was found as 0.12 according to the table. (N: 14 g / mol, H: 1 g / mol, Cl: 35.5 g / mol). Concentration (mg/L) Absorbance 0.01 5 0.05 7.5 0.1 10 0.15 12 0.18

A sample is analyzed, and its absorbance is measured to be (4.680x10^-1). Given that the [FeSCN2+]E is (7.79x10^-4), what is the value of the proportionality constant?    Answer in scientific notation if necessary.

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)?

A solution of a dye was analyzed by spectrophotometry, and the following calibration data were collected using a 1 cm cuvette. *graph in attachemnt*   Using the calibration data above for the dye solution, what is the dye concentration in a solution with an absorbance (A) = 0.52 if it was measured in a 1 cm cuvette?   Group of answer choices 3.0 x 10-6 M 6.0 x 104 M 2.0 x 10-6 M Not enough information is provided.

You diluted a concentrated dye by mixing 45 μL of the stock solution with 655μL of water and measured the absorbance at λmax. Using Beer’s law, youdetermined that the concentration of the dilute solution is 85 μg/mL. What wasthe concentration of the original solution.