GMU QUESTION 7An ethanol solution of 3.5 mg/100 ml of compound Y (150.0 g/mol) in a 1.00 cm quartz cell has an absorbance (A) of 0.972 at Amax-235nm. What is its molar extinction coefficient? Report your answer to the correct number of significant figures. Do not include units in youranswer.OGMU 2020

To calculate the molar extinction coefficient (ε) using the Beer-Lambert Law, we can use the…

Answered: GMU QUESTION 7 An ethanol solution of…

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter9: Atomic Absorption And Atomic Fluorescence Spectrometry

Section: Chapter Questions

Problem 9.1QAP

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Consider the reaction : A+B 2 AB. A calibration plot was constructed using x as the concentration for AB in M and y as the absorbance value of AB, it provided the linear equation : y=25x+0.0008. Determine the concentration of AB in M if the absorbance value is 1.22. Round and report your value to the THIRD decimal place. Numeric value only, no unit. No new data to sa IMG 0915.jpeg e to search PrtScn Home
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Concentration Fe(SCN)2+ (M) Absorbance 0.0001 0.386 0.0002 0.774 0.0003 1.154 0.0004 1.527 0.0005 1.931 Question 2 Analysis Section 1 1. Open a spreadsheet program, like Excel or Desmos, and plot your data points, with Absorbance on the y-axis and Concentration on the x-axis. 2. Fit a linear trendline and make sure the equation is labeled on your graph, including the R² value. 3. Fill in your equation below. Absorbance = -Concentration + The slope of your equation gives you the s-1 in the Beer's law equation: A = scl. Since I = 1 cm, the slope is equal to the ɛ of Fe(SCN)2+. The units of & are 1/(M*cm).
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