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Calculate mono isotopic mass and average mass of C8H10N4O2 , show your work .
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- Here are three fictitious elements and a molecular view of the atoms that compose them. The molar mass of the middle element, (b), is 25 grams per dozen (g/doz). (The atoms of these fictitious elements are much larger than ordinary atoms.) Based on the size of the atoms, do you expect the atomic masses of elements (a) and (c) to be greater than or less than (b)? How many atoms are present in 175 g of element (b)?Average Atomic Weight Part 1: Consider the four identical spheres below, each with a mass of 2.00 g. Calculate the average mass of a sphere in this sample. Part 2: Now consider a sample that consists of four spheres, each with a different mass: blue mass is 2.00 g, red mass is 1.75 g, green mass is 3.00 g, and yellow mass is 1.25 g. a Calculate the average mass of a sphere in this sample. b How does the average mass for a sphere in this sample compare with the average mass of the sample that consisted just of the blue spheres? How can such different samples have their averages turn out the way they did? Part 3: Consider two jars. One jar contains 100 blue spheres, and the other jar contains 25 each of red, blue, green, and yellow colors mixed together. a If you were to remove 50 blue spheres from the jar containing just the blue spheres, what would be the total mass of spheres left in the jar? (Note that the masses of the spheres are given in Part 2.) b If you were to remove 50 spheres from the jar containing the mixture (assume you get a representative distribution of colors), what would be the total mass of spheres left in the jar? c In the case of the mixture of spheres, does the average mass of the spheres necessarily represent the mass of an individual sphere in the sample? d If you had 80.0 grams of spheres from the blue sample, how many spheres would you have? e If you had 60.0 grams of spheres from the mixed-color sample, how many spheres would you have? What assumption did you make about your sample when performing this calculation? Part 4: Consider a sample that consists of three green spheres and one blue sphere. The green mass is 3.00 g, and the blue mass is 1.00 g. a Calculate the fractional abundance of each sphere in the sample. b Use the fractional abundance to calculate the average mass of the spheres in this sample. c How are the ideas developed in this Concept Exploration related to the atomic weights of the elements?In what way are isotopes of a given element always different? In what way(s) are they always the same?
- Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?A mass spectrometer determines isotopic masses to eight or nine significant digits. What limits the atomic mass of carbon to only five significant digits?2-17 How does Dalton’s atomic theory explain: (a) the law of conservation of mass? (b) the law of constant composition?
- The mass spectrum of bromine (Br2) consists of three peaks with the following characteristics: Mass (u) Relative Size 157.84 0.2534 159.84 0.5000 161.84 0.2466 How do you interpret these data?Rubidium has an atomic weight of 85.470 and two primary isotopes. The isotopes are rubidium-85 (84.9118 amu) and rubidium-87 (86.9092 amu). Calculate the abundance of each isotope. Show all work.121sb and 123Sb whose exact isotopic 23. The two naturally occurring isotopes of antimony are masses are 120.904 amu and 122.904 amu respectively. If the average atomic mass of Sb is 121.8 amu determine the percentage abundances of both isotopes. Show all your work and report your answer to appropriate significant figures.
- Silicon has only three stable isotopes. Calculate the atomic mass for silicon given the fact that 28Si (mass= 27.98 amu) has an abundance of 92.21%, 29Si (mass= 28.98 amu) has an abundance of 4.71% and 30Si (mass= 29.97 amu) at 3.09%. Please show your work as this is not a simple average, but a weighed average.Complete the table. Element Isotope No. of protons No. of neutrons Atomic mass (u) Isotopic abundance Ar (3 decimal places) 17Cl 35Cl 34.96885 75.5% 37Cl 36.96590 24.5% 29Cu 63Cu 62.92960 69.15% 65Cu 64.92779 30.85% 35Br 79Br 78.91834 50.8% 81Br 80.91629 49.2% 30Zn 64Zn 63.92914 49.17% 66Zn 65.92603 27.73% 67Zn 66.92713 4.04% 68Zn 67.92484 18.45% 70Zn 69.92532 0.61% 26Fe 56Fe 53.93961 5.845% 54Fe 55.93494 91.754% 57Fe 56.93539 2.119% 58Fe 57.93327 0.282%Calculate the average atomic mass of Amazium, a newly discovered element (Amazium, symbol Az) which is determined by mass spectrometry to have two isotopes with the following masses and percent (%) composition (abundance) Show work. Az-230 (mass = 229.995, % abundance = 45.23%) Az 236 (mass 235.989, % abundance = 54.77%) %3D Edit View Insert Format Tools Table 12pt v Paragraph v