See the answer. Convert grams Benzene to moles or moles Benzene to grams. What Is The Empirical Formula ? (Do not use the molar mass of the compound to find the empirical formula!) Molar mass of C6H6 = 78.11184 g/mol. a.) conversion of benzene is 95 % and the single pass conversion is 20 %, find the ratio of the recycle stream to the fresh feed stream as well as the composition of the product stream. Assume that 20 % excess hydrogen gas is used in the fresh feed. ›› Benzene molecular weight. The percentage by mass of hydrogen in benzene (C6H6) is 7.74%. Write the thermochemical equation for the combustion of one mole of C6H6 … The freezing point of benzene is 5.51 °C, and the K1 is 5.12 °C•kg/mol. mnormal = 94 . Sol. Benzene has the molecular formula C₆H₆, so there is an equal number of Carbon and Hydrogen per molecule 1:1. The vapor pressure of benzene is 95.1 torr and of toluene is 28.4 torr at this temperature. Analysis shows the compound to be 7.74% H by mass. Prob 15. A solution of benzene and toluene is 25% benzene by mass. or ( = 0.734 or 73.4 % . H2O (Dihydrogen monoxide) H= 1 g so 1 x2= 2 g O= 16 g so 16x1= 16 16+2=18 g total Next you divide each by the total 2 g H/ 18 g total= 0.111111 (x100)= 11.1% Hydrogen 16 g O/ 18 g toal=0.05555556(x100)= 88.9% Oxygen Note that the toal percent is 100 percent! Assuming ideal behavior, calculate each of the following: (a) Vapor pressure of each component. Benzene has a molar mass of 78.11 g/ mol. Give your answer regarding the composition as mass percent. Molecular weight calculation: 12.0107*6 + 1.00794*6 ›› Percent composition by element The molar mass of carbon is around 12.011 g / mol. The vapor pressures of pure benzene and pure toluene at 25 C are 94.2 torr and 28.4 torr, respectively. A 1.60 g sample of a mixture of naphthalene (C10H8) and anthracene (C14H10) is dissolved in 20.0 g benzene (C6H6). This problem has been solved! The freezing point of the solution is 2.81 °C. Kf for C6H6 = 5.120 mol(1kg. So I assumed 100 g. 7.74% => 7.74 g H. 78.1-7.74= 70.36 g C These Compounds Have The Same Percent Composition And Therefore The Same Empirical Formula. H has a molar mass of around 1.0079 g / mol. Prob 14. Example #5: Calculate the vapor pressure of a solution of 74.0 g of benzene (C 6 H 6) in 48.8 g of toluene (C 7 H 8) at 25.0 °C. Find the empirical and molecular formulas of benzene. We know that, (T = mexp = 148.41 . The combustion of 1.000g of benzene, C6H6 (l), in O2 (g) liberates 41.84kJ of heat and yields CO2(g) and H2O (l). As it contains only carbon and hydrogen atoms, benzene is classed as a hydrocarbon.. Benzene is a natural constituent of crude oil and is one of the elementary petrochemicals. I think what you’re getting confused about is the ratio of Carbon to Hydrogen. A solution containing 20 ( 10(3 kg of phenol in 1.0 kg of benzene has its f. pt depressed by 0.69 K. Calculate the fraction of phenol dimerised. ! 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