The vapour pressure, p, of nitric acid varies with temperature according to the following data table. 0/°C 20 40 50 70 80 90 100 p/kPa 1.92 6.38 17.7 27.7 62.3 89.3 124.9 170.9 Determine a) the normal boiling point and b) the enthalpy of vaporization of nitric acid.

The vapour pressure, p, of nitric acid varies with temperature according to the following data table. 0/°C 20 40 50 70 80 90 100 p/kPa 1.92 6.38 17.7 27.7 62.3 89.3 124.9 170.9 Determine a) the normal boiling point and b) the enthalpy of vaporization of nitric acid.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 122CP: Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution...

See similar textbooks

Similar questions

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/mol
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
At which temperature is the vapor pressure of ethanol equal to 80. kPa?
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.
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.
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 dichlorobenzene
The vapour pressure of pyridine is 50.0 kPa at 365.7 K and the normal boiling point is 388.4 K. What is the enthalpy of vaporization of pyridine?
The following temperature/composition data were obtained for a mixture of two liquids A and B at 1.00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapor at equilibrium 140 125 130 135 145 150 ТРС 0.91 0.65 0.45 0.30 0.18 0.098 ХА 0.99 0.91 0.77 0.61 0.45 0.25 The boiling points are 124 °C for A and 155 °C for B a) Plot the temperature composition diagram for the mixture. b) What is the composition of the vapor in equilibrium with the liquid of composition (i) 0.50, and (ii) x = 0.33? ХА
Aniline, C6H5NH2, and hexane, C6H14 , form partially miscible liquid - liquid mixtures at temperatures below 69. 1 °C. When 42.8 g of aniline and 75 .2 g of hexane are mixed together at a temperature of 67.5 °C, two separate liquid phases are formed, with mole fractions of aniline of 0.308 and 0.618.(a) Determine the overall mole fraction of aniline in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases.
A container is divided into two equal compartments. One contains 3.0 mol H2(g) at 25°C; the other contains 1.0 mol N2(g) at 25°C. Calculate the Gibbs energy of mixing when the partition is removed. Assume perfect behavior.
C6H5Cl e C6H5Br form nearly ideal mixtures. At 136.7◦ C the vapor pressure of C6H5Cl is 1.137 bar, while that of C6H5Br is 0.604 bar. Which is the composition of the mixture for which the total vapor pressure is 1 bar ?