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Nitrobenzene,
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General Chemistry: Principles and Modern Applications (11th Edition)
- Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/molarrow_forwardThe vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?arrow_forwardA forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?arrow_forward
- Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?arrow_forwardThe sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 calculated in part (ii) as a gas, calculate the pressure in the can when it is stored at 25 0C. (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093M)arrow_forwardConsider a body of water in equilibrium with solid calcium sulfate, CaSo4, for which Ksp= 3.0 x 10^-5 at 25 degrees C. Calculate the solubility, in g/L, of calcium sulfate in water assuming that other reactions are negligible. *arrow_forward
- s) At 20 °C the vapor pressure of benzene is 10 kPa and that of methylbenzene is 2.8 · kPa. If this mixture is an ideal solution, what is the total vapor pressure of an equimolar mixture of the two components? Note that equimolar means that there are the same number of moles of both substances.arrow_forwardWhat is the boiling point of the automobile radiator fluid prepared by mixing 1.02 Lof ethylene glycol (HOCH2CH2OH, density = 1.114 %3D g/mL) with 1.18 Lof water (density = 1.000 g/mL)? The Kp of water is 0.520°C/m. °Carrow_forwardIn a study designed to prepare new gasoline-resistant coat-ings, a polymer chemist dissolves 6.053 g of poly(vinyl alcohol)in enough water to make 100.0 mL of solution. At 25°C, the os-motic pressure of this solution is 0.272 atm. What is the molar mass of the polymer sample?arrow_forward
- The vapor pressure of water at 30 °C is 4.24 kPa. Calculate the vapor pressure if 95.0 g of xylose, C₅H₁₀O₅(l), is added to 100.0 mL of water. The density of water at 30 °C is 0.996 g・mL⁻¹.arrow_forwardwhat is the molar mass of toluene if 0.85g of toluent depresses freezing pt 1.00 x102 g of benzene by 0.47 degrees C; Kf=5.12degrees C/m.arrow_forwardA chemistry student is given 2.00 L of a clear aqueous solution at 42." C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 22.° C. At that point, the student sees that a precipitate has formed. He pours off the remaining liquid solution, throws away the precipitate, and evaporates the water from the remaining liquid solution under vacuum. More precipitate forms. The student washes, dries and weighs the additional precipitate. It weighs 0.400 kg. O yes Using only the information above, can you calculate the solubility of X in water at 22.C? O no If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits.arrow_forward
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