Calculate the vapour pressure at 80 degree C of a solution prepared by dissolvin
ID: 979894 • Letter: C
Question
Calculate the vapour pressure at 80 degree C of a solution prepared by dissolving 0.0300 moles of glucose in 100 g of water. The vapour pressure of water at 80 degree C is 355 Torr. 355 Torr 760 Torr 353 Torr 756 Torr 357 Torr Calculate the vapour pressure at 80 degree C of a solution prepared by dissolving 3.00 moles of glucose in 200.g of water. The vapor pressure pressure of water at 80 degree C is 355 Torr. 760 Torr 279 Torr 431 Torr 75.5 Torr 355 Torr The vapor pressure of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr, respectively, at 296 K. What is the (total) vapor pressure of a solution containing 50.0 g each compound? 460. Torr 274 Torr 260. Torr 33.0 Torr 241 Torr Which of the following 1.0 M solution contains the most particles? magnesium sulfide glucose ethylene glycol potassium chlorine All of the following have a van't Hoff i factor of 3 expert. calcium nitrate. magnesium chloride. ethylene glycol. barium hydroxide. sodium sulphate.Explanation / Answer
24) C) 353 torr
moles of glucose = 0.03 moles
moles of water = 100 / 18 = 5.56 moles
total moles = 0.03 + 5.56 = 5.586
mole fraction of water = 5.56 / 5.586 = 0.995
Vapor pressure of solution = Vapor pressure of water x mole fraction of water
= 355 torr x 0.995
=353 torr
25) B) 279 Torr
moles of glucose = 3 moles
moles of water = 200 / 18 = 11.11 moles
total moles = 3 + 11.11 = 14.11
mole fraction of water = 11.11 / 14.11 = 0.787
Vapor pressure of solution = Vapor pressure of water x mole fraction of water
= 355 torr x 0.787
= 279 torr
26) B) 274 torr
moles of CS2 = 50/ 76 = 0.658
moles of CCl4 = 50 / 154 = 0.325
mole fraction of CS2 = 0.658 / (0.658 + 0.325)
= 0.669
mole fraction of CCl4 = 0.331
P solution = (mole fraction CS2)(partial pressure CS2) + (mole fraction CCl4)(partial pressure CCl4)
= 0.669 x 360 + 0.331 x 99.8
= 274 torr
27) B) sodium sulfate
28) C) ehylene glycol
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