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Answer : c) 50g of sodium acetate in 200 mL of water due to maximum negative deviation of Rault's law.
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4) Which solution a, b or c has the highest vapor pressure? Calculate the vapor pressure...
Which solution has the highest vapor pressure? 0.75 mol of a volatile compound in 750 g...
Which solution has the highest vapor pressure? 0.75 mol of a volatile compound in 750 g of ethanol 0.75 mol of a nonvolatile compound in 750 g of ethanol Not enough information is given to determine which solution has the highest vapor pressure. 1.5 mol of a nonvolatile compound in 750 g of ethanol Solutions A and B have the same vapor pressure and it is higher than the vapor pressure of solution C.
Which of the following solutions will have the highest vapor pressure compared to the vapor pressure...
Which of the following solutions will have the highest vapor pressure compared to the vapor pressure of pure water at 25°C? ОА 0,1 mole of glucose, C6H12O6, dissolved in 1 kg of water. O B 0.1 mole of magnesium chloride dissolved in 1 kg of water. 0 C 0.1 mole of sodium hydrogen carbonate dissolved in 1 kg of water O D 0.1 mole of ammonium nitrate dissolved in 1 kg of water.
5. If you had 0.10 m solutions of each of the solutions in question #4, which would have: (hint, more ions cause bigger colligative properties, few particles in solution | K" ("C/m) Pur...
5. If you had 0.10 m solutions of each of the solutions in question #4, which would have: (hint, more ions cause bigger colligative properties, few particles in solution | K" ("C/m) Pure Solvents Water Ethanol Benzene | Ke rc/m ) 0.512 1.19 2.65 1.86 1.99 -5.12 will have a smaller colligative affect.) d. the highest vapor pressure? e. the lowest freezing point? a. the highest boiling point? b. the highest freezing point? c. the lowest osmotic pressure? 6. Calculate...
4.) Pure water has a vapor pressure of 31.1 torr at 30.1 °C. A solution is...
4.) Pure water has a vapor pressure of 31.1 torr at 30.1 °C. A solution is prepared by adding 90.8 g of unknown substance which is a nonvolatile and non-electrolyte to 375.0 g of water. The vapor pressure of the resulting solution is 29.5 torr. Calculate the molar mass of the unknown substance.
Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g...
Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g ethanol (M = 46 g/mol) in 500 mL of water. At 25 °C, the density of water is 0.9971 g/cm3 and the vapor pressure is 23.76 torr.
Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g...
Calculate the expected vapor pressure at 25 °C for a solution prepared by dissolving 235 g ethanol (M = 46 g/mol) in 500 mL of water. At 25 °C, the density of water is 0.9971 g/cm3 and the vapor pressure is 23.76 torr. 3.7 torr 20.06 torr 10.6 torr 12 torr
The vapor pressure if ethanol (C2H5OH) is 672 torr at 75°C. The vapor pressure of water...
The vapor pressure if ethanol (C2H5OH) is 672 torr at 75°C. The vapor pressure of water is 289 torr at the same temperature. Calculate the mole fraction of ethonal and water in a solution that is 12% ethanol by volume. Can any one help me step-by-step with this?
Problem #4: At 29.6 °C, pure water has a vapor pressure of 31.1 torr. A solution...
Problem #4: At 29.6 °C, pure water has a vapor pressure of 31.1 torr. A solution is prepared by adding 86.8 g of "Y", a nonvolatile non- electrolyte to 350. g of water. The vapor pressure of the resulting solution is 28.6 torr. Calculate the molar mass of Y.
9. At 304 K the vapor pressure of pure ethyl acetate (CH,COOC2Hs) is 0.173 atm and...
9. At 304 K the vapor pressure of pure ethyl acetate (CH,COOC2Hs) is 0.173 atm and the vapor pressure of pure methyl acetate (CH,CoOCH,) is 0.402 atm. Mixing 46.8 g of ethyl acetate M 68.11g/mo) with 45.8 g of methyl acetate (MM-74.08g/mol) gives a solution that is nearly ideal. (must show work to receive credit) (a) Calculate the mole fraction of ethyl acetate in the solution. XEl-acetate in solution (b) Calculate the total vapor pressure of the solution at 304...
5. Ethanol and methanol are form an ideal solution at 20 °C. Vapor pressure of pure...
5. Ethanol and methanol are form an ideal solution at 20 °C. Vapor pressure of pure ethanol and pure methanol at 20 °C is 44.5 and 88.7 mmHg, respectively. If 100 g of ethanol and 100 g of methanol are mixed into a solution, calculate: (a) the mol fractions of ethanol and methanol in the solution, (b) the partial pressures of ethanol and methanol and total pressure of the solution, and (c) the mol fraction of methanol in a vapor...
Which solution has the highest vapor pressure? 0.75 mol of a volatile compound in 750 g of ethanol 0.75 mol of a nonvolatile compound in 750 g of ethanol Not enough information is given to determine which solution has the highest vapor pressure. 1.5 mol of a nonvolatile compound in 750 g of ethanol Solutions A and B have the same vapor pressure and it is higher than the vapor pressure of solution C.
Which of the following solutions will have the highest vapor pressure compared to the vapor pressure of pure water at 25°C? ОА 0,1 mole of glucose, C6H12O6, dissolved in 1 kg of water. O B 0.1 mole of magnesium chloride dissolved in 1 kg of water. 0 C 0.1 mole of sodium hydrogen carbonate dissolved in 1 kg of water O D 0.1 mole of ammonium nitrate dissolved in 1 kg of water.
5. If you had 0.10 m solutions of each of the solutions in question #4, which would have: (hint, more ions cause bigger colligative properties, few particles in solution | K" ("C/m) Pure Solvents Water Ethanol Benzene | Ke rc/m ) 0.512 1.19 2.65 1.86 1.99 -5.12 will have a smaller colligative affect.) d. the highest vapor pressure? e. the lowest freezing point? a. the highest boiling point? b. the highest freezing point? c. the lowest osmotic pressure? 6. Calculate...
4.) Pure water has a vapor pressure of 31.1 torr at 30.1 °C. A solution is prepared by adding 90.8 g of unknown substance which is a nonvolatile and non-electrolyte to 375.0 g of water. The vapor pressure of the resulting solution is 29.5 torr. Calculate the molar mass of the unknown substance.
Problem #4: At 29.6 °C, pure water has a vapor pressure of 31.1 torr. A solution is prepared by adding 86.8 g of "Y", a nonvolatile non- electrolyte to 350. g of water. The vapor pressure of the resulting solution is 28.6 torr. Calculate the molar mass of Y.
9. At 304 K the vapor pressure of pure ethyl acetate (CH,COOC2Hs) is 0.173 atm and the vapor pressure of pure methyl acetate (CH,CoOCH,) is 0.402 atm. Mixing 46.8 g of ethyl acetate M 68.11g/mo) with 45.8 g of methyl acetate (MM-74.08g/mol) gives a solution that is nearly ideal. (must show work to receive credit) (a) Calculate the mole fraction of ethyl acetate in the solution. XEl-acetate in solution (b) Calculate the total vapor pressure of the solution at 304...
5. Ethanol and methanol are form an ideal solution at 20 °C. Vapor pressure of pure ethanol and pure methanol at 20 °C is 44.5 and 88.7 mmHg, respectively. If 100 g of ethanol and 100 g of methanol are mixed into a solution, calculate: (a) the mol fractions of ethanol and methanol in the solution, (b) the partial pressures of ethanol and methanol and total pressure of the solution, and (c) the mol fraction of methanol in a vapor...
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