5A. Sorbitol, used as a sweetener in some sugar-free foods, has a molecular mass of 182 u and a mass percent composition of 39.56% C, 7.74% H, and 52.70% O. What are the empirical and molecular formulas of sorbitol? ? (Mc=12.011g/mol, Mµ= 1.008 g/mol and Mo= 15.999 g/mol)

74. A throat lozenge contains 5.0 mg of menthol, which has the formula C10H20O. How many moles of menthol are in 5.0 mg of menthol? What is the mass in grams of 1.56 moles of menthol? 79. For each of the following ionic substances (a) Co2O3 and (b) Fe2(C2O4)3, calculate its formula mass and write a conversion factor that converts between mass in grams and moles of the substance.

5.) Ethylene glycol is a coolant widely used in automobiles. If its molecular formula is C2H6O2, how many moles would be present if you had 2500 g of this in your vehicle? A) 1.6 x 105 mol B) 2.5 x 10-2 mol C) 62 mol D) 40. mol

2. Fermentation is a complex chemical process of making wine by converting glucose into ethanol and carbon dioxide: C2H5OH) + CO2(g) Calculate the mass of ethanol produced if 600.0 grams of glucose reacts completely. C6H12O6(s) 3. Consider the reaction of zinc metal with hydrochloric acid, HClçaq). Zns) + 2 HCl(aq) > ZnClz(aq) + Hz(g)

Conine (M = 127.23 g/mol), a substance isolated from poison hemlock, contains only carbon, hydrogen, and nitrogen. Combustion of 5.024 mg of conìine yields 13.90 mg COz and 6.048 mg of H2O. What are the empirical and molecular formulas ofconine?

8) Camphor is an organic compound extracted from the camphor laurel tree. Its strong aroma makes it a common ingredient in many cooking recipes and perfumes. It contains C, H, and O. The combustion analysis of an 8.006 g sample of camphor affords 23.136 g of carbon dioxide and 7.579 g of water. The molecular weight of camphor is between 150 and 160 g.mol¹. a. What is the mass of carbon originally present in the tartaric acid sample?  b. What is the mass of hydrogen originally present in the tartaric acid sample?  C. What is the mass percentage of C, H and O in tartaric acid?  d. What is the empirical formula of tartaric acid?

1. Urea can be prepared by reacting ammonia with carbon dioxide.                               2 NH3 (g) + CO2 (g) ® (NH2)2C=O (aq) + H2O (l)    Calculate the mass of urea (in grams) which is formed from the reaction of 375 g of ammonia with 650 g of CO2.

2. A hydrocarbon was found to be 20% hydrogen by mass. If the molar mass is 30 g/mol, what is the molecular formula? А. СH В. СН C. CH3 D. C,H4 E. C2H. 3. If one mole of ammonium perchlorate is allowed to react with excess aluminum, how many molecules of water will be produced? 3NH,C1O, + 3A1 Al,O, 3NO 6H2O А. 3.61 x 1023 В. 1.00 х 1023 C. 6.02 x 1023 D. 1.20 x 1024 E. 3.01 x 1024 4. A mixture containing 0.40 mol Al in contact with 0.75 mol Cl, is ignited in a closed container. Assum ing complete reaction, which gives the maximum quantity of AICI, produced and quantity of unconsumed reactant? A. 0.40 mol AICI, and 0.15 mol Al unreacted B. 0.40 mol AICI, and 0.15 mol Cl, unreacted C. 0.40 mol AICI, and 0.35 mol Cl, unreacted D. 0.50 mol AICI, and 0.10 mol Alunreacted E. 0.50 mol AICI, and 0.15 mol Cl, unreacted

10)

Valproic acid, a medication used to treat epilepsy and bipolar mania, contains only C, H, and O. Combustion of 1.000 g of valproic acid produces 2.441 g of CO₂ and 1.000 g of H₂O. Determine the molar mass of the compound if it is between 80.0 and 150.0 g/mol. Provide an answer to four significant figures.