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- The vapor pressure of a substance at 20.0 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol-1. Estimate the temperature at which its vapor pressure is 66.0 kPa.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.Refer to Fig. 4A.8. Describe the phase or phases present as the pressure on a sample of CO2 is steadily increased from 0.1 atm: (a) at a constant temperature of 200 K; (b) at a constant temperature of 310 K; (c) at a constant temperature of 216.8 K.
- Consider a system where 2.40 mol of CH3CN(g) are converted into CH3CN(1) at 1.00 atm and 82.0 °C. The normal boiling point of CH3CN is 82.0 °C, and AvapH much less than the volume of CH3CN(g). 29.75 kJ mol-1. Assume the volume of CH3CN(I) is What is the enthalpy change for the process described above? Enter your answer in kilojoules accurate to three significant figures. Do not use scientific/exponential notation. AH= Number kJ. What is the work done during the process described above? w= -7087.0 J w= 798.2 J w= -69.9 J w = 69.9 ) w = 7087.0 J O O O(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?The Clausius- Clapeyron equation on the assumption that the enthalpy of vaporization is independent of temperature in the range of interest. (a) Theenthalpy of vaporization of water is 40.656 kJ mol-1 at its normal boiling temperature, 373 K. Assuming that the enthalpy of vaporization does not vary with temperature, calculate the vapour pressure of water at 308 K. (b) Derive an improved version of the equation on the basis that the enthalpy of vaporization has the form ΔvapH =a+ bT. (c) For water in the range298- 373 K, a= 57.373 kJ mol-1 and b = -44.801 J K-1 mol- 1. Use your improved version of the Clausius-Clapeyron equation to calculate a more reliable value for the vapour pressure of water at 308 K.
- 5C. 2(b) Sketch the phase diagram of the system of NH/NH, given that the two substances do not form a compound; NH, freezes at -78 °C; N₂H, freezes at 2 °C; a eutectic is formed when the mole fraction of N H is 0.07; and the eutectic melts at -80 °C.Refer to Fig. 4A.8. Describe the phase or phases present as a sample of CO2 is heated steadily from 100 K: (a) at a constant pressure of 1 atm; (b) at a constant pressure of 70 atm.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 vapour pressure of hexane between -10°C and +90°C fits the expression log(p/Torr) = 7.724 – 1655/(T/K). Calculate the enthalpy of vaporization.A solution containing 1.470 g of dichlorobenzene in 50.00 g of benzene boils at 80.60 degree C and a pressureof 1.00 bar. The boiling point of pure benzene is 80.09 degree C, and the molar enthalpy of vaporization of purebenzene is 32.0 kJ/mol. Determine the molecular mass of dichlorobenzeneA handbook lists the normal boiling point of isooctane, a gasoline component, as 99.2ºC and its enthalpy of vaporization as 35.76 kJ mol-1. Calculate the vapor pressure of isooctane at 25ºC.