Ahypothetical solution forms between a solid and a liquid The values of the themodyn Involved in the process are shown in the following table Action Enthalpy 14.5k/mol 21.8kJ/mol separation of solute separation of solvent formation of solute-solvent interactions-85.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute Enter your answer numerically in kilojoules per mole of solute.

A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 12.5 kJ/mol separation of solvent 28.8 kJ/mol formation of solute-solvent interactions -88.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute. Enter your answer numerically in kilojoules per mole of solute.

The freezing point of a CaCl₂ solution formed by dissolving 0.020 mol of CaCl₂ in 1,090 g of H₂O is-0.0397 °C. CaCl₂ dissociates as follows: Data: Ky 1.86 kg.K/mol The % dissociation, rounded to two significant figures, of CaCl₂ is: Number CaCl₂ Ca²+2 Ch %

Determine the osmotic pressure of a 119.1 L aqueous solution that contains 3.1 g of NaI  at 23 C. The molar mass of NaI is 149.89 g/mol. R = 8.314 J/mol*K or 0.0821 L*atm/(mol*K) Round your answer to contain two significant figures.   Your Answer:

Which of the following three solute/solvent pairs are insoluble? Choose one or more: benzene/toluene Benzene Toluene acetone/ammonia Acetone H. N. H. Ammonia mercury/water Hg Mercury O. H. Water O butane/ethanol Butane H. Ethanol water/xylene H' H. Water Xylenes propane/octane Propane Octane

Moles of solute (mol)Use the molality to convert kg of solvent to moles of solute.   Hints: molality of the solution (m) 0.76612903225806 Mass of solvent in grams 151.5 Mass of solvent in kilograms 0.1515

(Q73) A solution contains 16.90 grams of magnesium chloride and 815.7 grams of water. What is the vapor pressure (in torr) of this solution at 40.00°C? The vapor pressure of water at this temperature is 55.30 torr. You should use the experimental value of the van't Hoff factor for this calculation. (4 sf)

Given: Mass of lauric acid (g): 8.000g Mass of benzoic acid (g): 1.027g Freezing temperature of pure lactic acid(°C): 43.3°C Freezing point of the benzoic acid-lauric acid mixture(°C): 39.8°C m of lauric acid: 1.8m Mols of benzoic acid solute: .0072mol Question: Calculate the experimental molecular weight of benzoic acid, in g/mol.

What is the boiling point of a solution that contains 1.00 kg of water and each of the following quantities of solute?a. 2.00 moles of sucrose (a molecular compound) b. 2.00 moles of fructose (a molecular compound) c. 2.00 moles of Na2SO4 (an ionic compound) d. 2.00 moles of KCl (an ionic compound)

Calculate the freezing point of a solution containing 74.0 g of eucalyptol (C10H8O) solute dissolved in 0.600 kg of CHCl3.  The freezing point of pure CHCl3 is -63.5 oC.  CHCl3 has a Kf of 4.68 oC/molality. -64.9 oC -67.5 oC -48.3 oC -58.0 oC -69.0 oC -62.1 oC -59.5 oC -78.7 oC