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At an unknown temperature a solution made of (5.180x10^0) g of a non-volatile solute dissolved in...
1f. At an unknown temperature a solution made of (7.740x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.51x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.360x10^1) g/mol. 1g. A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor...
1e. An aqueous solution has a mole fraction of solute of (4.73x10^-2). The density of the solution is (1.1400x10^0) g/mL and the solute has a molar mass of (8.020x10^1) g/mol. What is the Molarity of solute of this solution? 1f. At an unknown temperature a solution made of (7.740x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.51x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at...
6. Please help is due in 30 mins, will rate, Thank you! At an unknown temperature a solution made of (6.550x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.21x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (4.080x10^1) g/mol.
When (8.61x10^1) g of a non-electrolyte is dissolved in (5.3100x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the molar mass (in g/mol) of the non- electrolyte solute? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to...
19.193 g of a non-volatile solute is dissolved in 180.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 20°C the vapour pressure of the solution is 17.242 torr. The vapour pressure of pure water at 20°C is 17.535 torr. Calculate the molar mass of the solute (g/mol). Now suppose, instead, that 19.193 g of a volatile solute is dissolved in 180.0 g of...
An aqueous solution has a mole fraction of solute of (3.660x10^-2). The density of the solution is (1.20x10^0) g/mL and the solute has a molar mass of (8.3800x10^1) g/mol. What is the Molarity of solute of this solution? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...
Vapour Pressure of Solutions of Non-Volatile or Volatile Solutes 31.686 g of a non-volatile solute is dissolved in 460.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 10°C the vapour pressure of the solution is 9.055 torr. The vapour pressure of pure water at 10°C is 9.209 torr. Calculate the molar mass of the solute (g/mol). See example 17.1 on pp865-6 of Zumdahl...
17.298 g of a non-volatile solute is dissolved in 265.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 519.57 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol).
When 8.59 g of an unknown, non-volatile, non-electrolyte, X was dissolved in 100. g of benzene, the vapor pressure of the solvent decreased from 100 torr to 97.5 torr at 299 K. Calculate the molar mass of the solute, X.