When 780 g of benzene (Molar mass = 78 g/mol) reacts with 750 mL of concentrated HNO3 (16 M) and 750 mL of H2SO4 (18 M), 1000 g of nitrobenzene (molar mass = 123 g/mol) and 250 g of an unknown compound with a high boiling point are obtained.
c. Give the name of the most probable side product with the high melting point. Explain why.
e. Supposing the crystalline compound (250 g) has the formula C6H4N2O4, calculate the yield of this side product. (Please show work..what are you using as the limiting reagent?)
When 780 g of benzene (Molar mass = 78 g/mol) reacts with 750 mL of concentrated...
4. When 10 g of benzene (Molar mass 78 g/mol) reacts with 9 mL of concentrated HNO3 (16 M) and 9 mL of H2SO4 (18 M), 8.1 g of nitrobenzene (molar mass 123 g/mol) and 1.2 g of an unknown compound with a high boiling point are obtained. a. Identify the limiting reagent. b. Calculate the percent yield of nitrobenzene. c. Give the name and structure of the most probable side product with the high melting point. d. Explain, with...
Pure benzene, C6H6, has a molar mass of 78.114 g mol-1, a density of 0.8765 g mL-1, a freezing point of 5.45°C, and a boiling point of 80.2°C. Its freezing point depression and boiling point elevation constants are: Kf = 5.07°C m-1; Kb = 2.53oC m-1. A solution was made by taking 33.88 g of an unknown nonelectrolyte and dissolving it in 175.0 g of benzene. The measured freezing point of the solution was 1.65oC. Calculate the molar mass of...
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
Ester= Isoamyl acetate (banana) Molar mass of banana= 130.19 density= 0.876 g/ml 5.26 g ester product. Alcohol= isoamyl alcohol density= 0.81 g/ml Molar mass= 88.148 g/mol Quantity= 5.4 ml Carboxylic acid= acetic acid density= 1.05 g/ml Molar mass= 60.052 g/mol Quantity= 11.4 ml and 1 ml of concentrated H2SO4 (1.8 g, 0.018 mole) was also used in the procedure. Calculate theoretical yield and % yield .
The molar mass of a nonelectrolyte is 58.0 g/mol. Compute the boiling point of a solution containing 16.9 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.725 °C.
What is the boiling point when 14.09 g of aspirin (a molecular compound with a molar mass = 176.60 g/mol) is dissolved in 199.10 g of benzene (solvent)?
Physical Properties of Regents and Products Molar Structure and Mass Density Melting Formula (g/mol) (g/mL) Pt. (°C) Name Boiling Pt. (°C) (1) cis-stilbene (2) trans-stilbene (3) pyridinium tribromide (4) Glacial Acetic Acid
Physical Properties of Regents and Products Name Structure and Formula Molar Mass (g/mol) (g/mL) Melting PL (C) Boiling PL. () (1) Ethyl acetoacetate (2) Sucrose (3) Disodium hydrogen phosphate (4) Sodium borohydride (5) Ethyl-3- hydroxybutyrate Quantities of Reagents Used and Products Formed Structural Formula Mass Moles Volume (ml)
Physical Properties of Regents and Products Name Structure and Formula Molar Mass (g/mol) Density (g/mL.) Melting Pl(C) Boiling PL. (°C) (1) Ethyl acetoacetate (2) Sucrose (3) Disodium hydrogen phosphate (4) Sodium borohydride (5) Ethyl-3- hydroxybutyrate Quantities of Reagents Used and Products Formed Structural Formula Moles Volume Volume (mL) Mass
The molar mass of a nonelectrolyte is 58.0 g/mol. Compute the boiling point of a solution containing 22.7 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.725 °C.