1. The vapour pressure of CCl4 at 20°C is 11.9 kPa and its enthalpy of vaporization is 33.0 kJ mol-¹. What is its standard boiling temperature?
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![1. The vapour pressure of CCl4 at 20°C is 11.9 kPa and its enthalpy of vaporization
is 33.0 kJ mol-¹. What is its standard boiling temperature?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12f51b64-c3b4-40b6-b565-16b387e10bf1%2F142487ec-30ad-4187-8202-346c1cb0c5b3%2Fjaj2rwl_processed.png&w=3840&q=75)
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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 vapor pressure of a liquid between 15 C and 35 C fits the expression log(p) = 8.750 – 1625/T with p in Torr and T in K. Calculate (i) the enthalpy of vaporization and (ii) the normal boiling point of the liquid.Step by step pls
- 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?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.
- 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.A 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.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 dichlorobenzeneThe enthalpy of vaporization of a certain liquid is found to be 14.4 kJ mol−1 at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are 115 cm3 mol−1 and 14.5 dm3 mol−1, respectively. (a) Use the Clapeyron equation to estimate dp/dT at the normal boiling point. (b) If the Clausius–Clapeyron equation is used instead to estimate dp/dT, what is the percentage error in the resulting value of dp/dT?
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