Carbon tetrachloride (CC14) has a normal boiling point of 75.38 °C, and an enthalpy of vapourization (AvapH) of 32.31 kJ.mol-¹. What will its vapour pressure be at 28.3 °C (in kPa)? (Use two decimal places)
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- 3. A 12.0 cm3 sample of liquid H2O (density 1.00 g.cm-3) is heated to 328 oC under an external pressure of 0.8 atm, conditions under which it vapourises: (i) Calculate the volume of the gas. (ii) Calculate the mass of the same volume (as in part i) of CO2 gas under the same conditions. (iii) Calculate temperature of that sample of CO2 (as in part ii) at 8.0 atm pressure in a 20.0 L container.The standard enthalpy of vaporization (H°vap) of ethylenediamine ((NH2CH2)2) is 44.0 kJ/mol.The normal boiling point of ethylenediamine is 116.5°C.Calculate the vapour pressure of ethylenediamine at 102.0°C.The ΔH°soln of HNO3 is –33.3 kJ/mol. 11.0 mL of 14.0 M HNO3 is dissolved in 100.0 mL of distilled water initially at 25°C. How much ice at 0°C [cP = 37.1 J/(mol ·°C), ΔH°fus = 6.01 kJ/mol] must be added to return the solution temperature to 25°C after dissolution of the acid and equilibrium with the ice is reached? The molar heat capacity is 80.8 J/(mol·°C) for the solution, and the molar heat capacity is 75.3 J/(mol·°C) for pure water.
- The vapour pressure of a liquid at 35°C is 0.60 bar and its enthalpy of vaporization is 40 kJ/mol. What is the boiling point of this liquid (in °C) at the atmospheric pressure of 1.00 bar?Which has the greatest vapour pressure at 25°C? SiO2 CO2 H2OAt which temperature is the vapor pressure of ethanol equal to 80. kPa?
- (i) 578,070 J of heat is requred to raise the temperature of 15.0 moles of liquid methanol, CH3OH, from 25.0 °C to its boiling point (64.6 °C) and then to completely evaporate the methanol at that temperature. The specific heat of liquid methanol is 2.53 J g-1 K-1 vaporisation of the compound. Calculate the enthalpy of vapourisation of the compound?Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mLAt 25 °C, the equilibrium vapour pressure of ethanol is 0.0821 bar. The standard enthalpy of vapourization is 39.28 kJ/mol. What is the boiling point of ethanol at standard pressure? In other words, at what temperature does the equilibrium vapour pressure of ethanol reach 1.000 bar? Report your answer in degrees Celsius, but do not include the units in the answer. Report your answer to the nearest degree.
- Suppose you have 600.0 grams of room temperature water (20.0 degrees Celsius) in a thermos. You drop 90.0 grams of ice at 0.00 degrees Celsius into the thermos and shut the lid.(a) What is the equilibrium temperature of the system? (b) How much ice is left (in grams)? Provide a step-by-step explanation for how you arrived at your solution as though you were teaching a student to solve this type of problem.The standard enthalpy of vaporization (H°vap) of diethylether ((CH3CH2)2O) is 29.1 kJ/mol.The normal boiling point of diethylether is 34.5°C.Calculate the vapour pressure of diethylether at 19.0°C. (Units of pressure can be atm, torr, mmHg, Pa, kPa, bar, etc. -- units are always case sensitive)What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.