Two of the compounds shown give the base peak at m/z 43 in the mass spectrum. Which two are they? ✰ ✰ ✰ ✰ 3 A. 1 and 2 C. 1 and 4 D. 2 and 3 E. 2 and 4 B. 1 and 3 F. 3 and 4
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- When LC is coupled with mass spectrometry (MS), what are the advantages (compared to LC only) in terms of analyte identification and quantitation in the sample?2. Which of the following isotopes contributes the tallest (most abundant) [M+1]* peak in mass spectrometry? 81 Br 13C 37C1 D(H) A. B. C. D.The ppm concentration of Pb2+ in a blood sample were measured with Spectrophotometry. 5.00 mL of a blood sample were taken and this sample gave a signal of 0.301 a.u.. Another 5.00 mL of a blood sample were mixed with 0.50 mL og 1.75 ppm Pb2+. Then, this mixture was diluted to 25.00 mL and this diluted mixture gave a signal of 0.406 a.u.. What is the ppm concentration of a blood sample?
- 30. (6) Determine four molecular formulas for a compound with a mass spectrum of 180: 182 (M: M+2) in a 3:1 ratio. (b) Calculate DBEs for each formula.Explain why is FAAS a good method of quantifying Ca in milk?Q.1. Predict the relative intensity of the M, M+1, and M+2 peaks for a low resolution mass spectrum of a compound with molecular formula, C6H13Br. The natural abundances of the select isotopes are given below. 35 Cl: 75.8% 79Br: 50.5% 12C: 98.89% 37Cl: 24.2% (The ratio is almost 3:1) 81Br: 49.5% (The ratio is almost 1:1) 13C: 1.11%
- 16. Based upon the following mass spectral data, what is the correct formula of the compound that generated the data? m/z 119 Rel. Int. (%) 100 120 5.9 121 32 a) CHNBR b) C5H10CIN c) C3H,N d) C4H11N2O2 e) C4H&CIN2d. dipôle moments between atoms. The mass spectrum of CH3F is given in the chart below. (a) Draw a likely structure for the molecular ion (m/z 34). (b) Assign structural formulas to the two other high abundance peaks (m/z 33 and m/z 15) in the spectrum. (c) Propose an explanation for the low abundance of the peak at m/z 19. Relative lon Abundance 100 80 60 40 20 _________g 10 15 MW: (g/mol) C=12 H₂= 3 F: 19 20 25 miz 30 35Chemistry Common Isotopes and Mass spectrum of element Mo are given below Most common isotopes: Mo-98; Mo-96 Mo-95; Mo-92; Mo-97 ; Mo-100; Mo-94 Calculate the average atomic mass of Mo How the MS determined the relative intensity (Scale of 100) and Isotope abundance (%)? Why absolute intensity was not used? Can detector sensitivity, ICPMS temperature influence the relative intensity? Explain
- Q5. Figure 2 shows the mass spectrum of the same compound from an El source and a Cl source. (a) Which mass spectrum would be best for determining the molecular mass of the compound? Why? (b) Which mass spectrum would be best for determining the chemical structure? Why? (c) The El source was a pulsed source used with a TOF mass analyzer. If the flight tube were 1.0 m long and the accelerating volt age were 3000 V, what would the flight time be for the ion at m/z = 58? Relative abundance 100 80 60 40 20 0 T 50 58 69 ul 100 m/z 150 200What is a characteristic feature of halogens on the mass spectrometry spectra? A. They have abundant isotopic peaks B. They have m/z values less than 100 C. They do not show up on mass spectrometry D. They possess at least 10 peaks with equal intensityUnknown compound D has a melting point of 102-3C. Carbon/hydrogen analysis of compound D showed 30.4% carbon and 2.1% hydrogen. A Carius sulfur analysis of a 8.45-mg sample of compound D yielded 8.32 of BaSO4. A 10.50-mg sample of compound D was reacted in a sodium fusion reactor and the resulting solution produced 8.32 mg of AgBr. Based on mass spectral data, the M+ peak was found to be approximately 235 - 240 . Treatment of compound D with aqueous acid and heat yielded a compound with the formula C6H5Br Determine the molecular formula for compound D.