Calculate the mass percentage of benzene

Learning Objectives • To describe the concentration of a solution in the way that is most appropriate for a particular problem or application. There are several different ways to quantitatively describe the concentration of a solution. For example, molarity was introduced in Chapter 4 as a useful way to describe solution concentrations for reactions that are carried out in solution. Mole fractions, introduced in Chapter 10, are used not only to describe gas concentrations but also to determine the vapor pressures of mixtures of similar liquids. Example 4 reviews the methods for calculating the molarity and mole fraction of a solution when the masses of its components are known. Example 4 Commercial vinegar is essentially a solution of acetic acid in water. A bottle of vinegar has 3.78 g of acetic acid per 100.0 g of solution. Assume that the density of the solution is 1.00 g/mL. • What is its molarity? • What is its mole fraction? Given: mass of substance and mass and density of solution Asked for: molarity and mole fraction Strategy: • Calculate the number of moles of acetic acid in the sample. Then calculate the number of liters of solution from its mass and density. Use these results to determine the molarity of the solution. • Determine the mass of the water in the sample and calculate the number of moles of water. Then determine the mole fraction of acetic acid by dividing the number of moles of acetic acid by the total number of moles of substances in the sample. Sol...

Mass of solution = Mass of benzene + Mass of barbon tetrachloride = 22 g + 122 g = 144 g Mass percentage of benzene = Mass of benzene Mass of solution × 100 = 22 g 144 g × 100 = 15.28 % Mass percentage of CCl 4 = Mass of CCl 4 Mass of solution × 100 = 122 144 × 100 = 84.72 % Alternatively, mass percentage of CCl 4 = 100 − Mass percentage of benzene = 100 − 15.28 = 84.72 %.

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:A solution of benzene (C_6H_6) and toluene (C_7H_s) is 24.0 % benzene by mass. The vapor pressures of pure benzene and pure toluene at 25 degree C are 94.2 and 28.4 torr, respectively. You may want to reference pages 497 - 507) Section 12 6 while completing this problem Assuming ideal behavior, calculate the mass percent of benzene in the vapor. Express A solution of benzene (C_6H_6) and toluene (C_7H_s) is 24.0 % benzene by mass. The vapor pressures of pure benzene and pure toluene at 25 degree C are 94.2 and 28.4 torr, respectively. You may want to reference pages 497 - 507) Section 12 6 while completing this problem Assuming ideal behavior, calculate the mass percent of benzene in the vapor. Express the mass percent to three significant figures. Previous question Next question

More information on molar mass and molecular weight In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together. A common request on this site is to The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular weight), which is based on isotropically weighted averages. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass. Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction. These relative weights computed from the chemical equation are sometimes called equation weights. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance. Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms i...