(a)The normal boiling point of water is 100.0C.Its vapor pressure at 90C is 525.76 mm Hg.Calculate the enthalpy of vaporization of water(kJ mol). )贤 thus,AH.=RIn (P儿TT, =8341 Ko'(725g0+2771m+2 1 1 =41.5×103Jmol- =41.5kJ mol-1 (b)10.0g of dissolved in 1 kg of water.Calculate the vapor pressure of this solution at 90C 2(23.0)+321+64gmor=0.0704mol→021 molions 10.0g 1kg water= 18.0gmoFT=55.5mol 1000g 55.5 X0-55+02m=0,96 Pu4,0=p°4，oX4,o=525.76mmHg(0.996)=523.77mmHg 3. (a)Kp for the equilibrium FeOs)+COFe(s)+CO2 at 1000C is 0.403.If CO()at a pressure of 1.000 atm and excess FeO are mixed in a container at 1000C,what are the partial pressures of CO and CO)when equilibrium is attained? Initial,atm 1.00 0 Change,atm x +x Equilibrium,atm 1.00-x 4 4 2. (a) The normal boiling point of water is 100.0o C. Its vapor pressure at 90o C is 525.76 mm Hg. Calculate the enthalpy of vaporization of water (kJ mol-1). 2 vap 1 1 2 1 2 vap 1 12 1 1 3 1 1 p H 1 1 ln p R TT p 1 1 thus, H R ln p TT 760mmHg 1 1 8.314 J K mol ln 525.76 90 273K 100 273K 41.5 10 J mol 41.5kJ mol − − − − − ⎛⎞ ⎡ ⎤ Δ ⎜ ⎟ = − ⎢ ⎥ ⎝⎠ ⎣ ⎦ ⎛ ⎞⎡ ⎤ Δ= − ⎜ ⎟⎢ ⎥ ⎝ ⎠⎣ ⎦ ⎛ ⎞⎛ = − ⎜ ⎟⎜ ⎝ ⎠⎝ + + = × = ⎞ ⎟ ⎠ (b) 10.0 g of Na2SO4(s) is dissolved in 1 kg of water. Calculate the vapor pressure of this solution at 900 C. 2 2 22 1 1 H O 0 HO HO HO 10.0g 0.0704mol 0.211molions 2(23.0) 32.1 64g mol 1000g 1kg water 55.5mol 18.0g mol 55.5 X 0.996 55.5 0.211 p p X 525.76mmHg(0.996) 523.77 mmHg − − = → + + = = = = + == = 3. (a) Kp for the equilibrium FeO(s) + CO(g) ∩ Fe(s) + CO2(g) at 1000o C is 0.403. If CO(g), at a pressure of 1.000 atm and excess FeO(s) are mixed in a container at 1000o C, what are the partial pressures of CO(g) and CO2(g) when equilibrium is attained? CO(g) CO2(g) Initial, atm 1.00 0 Change, atm -x +x Equilibrium, atm 1.00-x x