Appl Of Ms Excel In Analytical Chemistry
2nd Edition
ISBN: 9781285686691
Author: Crouch
Publisher: Cengage
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6. This question refers to the compound aluminum sulfate octadecahydrate, Al2(SO4)3-18H₂O. Report
your answers to parts (a)-(c) to 2 decimal places.
(a) Calculate the formula weight.
(b) What is the percent water in the compound?
(c) What is the percent oxygen in the compound?
(d) How many atoms of hydrogen are present in 1.00 g of the compound? Report your answer
in scientific notation to 3 significant figures.
(a) Calculate the molar mass of ammonium nitrate, NH4NO3. (b) What is the mass percent of nitrogen in ammonium nitrate? (c) How many kilograms of nitrogen are present in a 10.0-lb bag of ammonium nitrate? (d) How many kilograms of ammonium nitrate contain 1.00 lb of nitrogen? (1 lb = 453.6 g)
Answer true or false.
(b) Avogadro’s number, to three significant figures, is 6.02 x 1023 formula units per mole.
(d) 1 mol of H2O contains 3 x 6.02 x 1023 formula units.
(i) 1 mol of ibuprofen, C13H18O2, contains 33 mol of atoms.
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 4-53 A typical deposit of cholesterol, C27H46O, in an artery might have a mass of 3.9 mg. How many mol ecules of cholesterol are in this mass?arrow_forward4-102 Aspartame, an artificial sweetener used as a sugar substitute in some foods and beverages, has the molecular formula C14H18N2O5. (a) How many mg of aspartame are present in 3.72 × 1026 molecules of aspartame? (b) Imagine you obtain 25.0 mL of aspartame, which is known to have a density of 1.35 g/mL. How many molecules of aspartame are present in this volume? (c) How many hydrogen atoms are present in 1.00 mg of aspartame? (d) Complete the skeletal structure of aspartame, where all the bonded atoms are shown but double bonds, triple bonds, and/or lone pairs are missing. (e) Identify the various types of geometries present in each central atom of aspartame using VSEPR theory. (f) Determine the various relative bond angles associated with each central atom of aspartame using VSEPR theory. (g) What is the most polar bond in aspartame? (h) Would you predict aspartame to be polar or nonpolar? (i) Is aspartame expected to possess resonance? Explain why or why not. (j) Consider the combustion of aspartame, which results in formation of NO2(g) as well as other expected products. Write a balanced chemical equation for this reaction. (k) Calculate the weight of C02(g) that can be prepared from 1.62 g of aspartame mixed with 2.11 g of oxygen gas.arrow_forward4-78 (Chemical Connections 4A) How does fluoride ion protect the tooth enamel against decay?arrow_forward
- You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.arrow_forwardFig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.arrow_forwardWhich molecule has a molecular mass of 28.05 amu?arrow_forward
- 4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.arrow_forward4-49 Calculate the number of: (a) nitrogen atoms in 25.0 g of TNT, C7H5N3O6 (b) carbon atoms in 40.0 g of ethanol, C2H6O (c) oxygen atoms in 500. mg of aspirin, C9H8O4 (d) sodium atoms in 2.40 g of sodium dihydrogen phosphate, NaH2PO4arrow_forwardDetermine the mass of each of the following:(a) 0.0146 mol KOH(b) 10.2 mol ethane, C2H6(c) 1.6 × 10−3 mol Na2 SO4(d) 6.854 × 103 mol glucose, C6 H12 O6(e) 2.86 mol Co(NH3)6Cl3arrow_forward
- 3) An organic compound contains only C, H, and O. Complete combustion of a 3.185 g sample in an excess of oxygen yields 8.846 g CO2 and 2.507 g H2O. (a) What is the percent composition, by mass, of this compound? (b) What is the empirical formula of the compound? (c) If the molar mass of this compound is 206 g/mol, what is the molecular formula? (C: 12.01 g/mol; H: 1.01 g/mol; O: 16.0 g/mol)arrow_forward4. (a) What is the difference between adding subscript 2 to the end of the formula for CO to give CO2 and adding a coefficient in front of the formula to give 2CO? (b) Is the following chemical equation, as written, consistent with the law of conservation of mass? 3Mg(OH)2 (s) + 2H3PO4 (aq) Why or why not? Mg3(PO+)2 (s) + H2O (I)arrow_forwardThe molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6H10OS2. (a) What is the molar mass of allicin? (b) How many moles of allicin are present in 5.00 mg of this substance?arrow_forward
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