Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY is -595.6 kJ mol1.The hydration energy of its ions is -612.4 kJ mol 1. Write the thermochemical equations for the two steps in the formation of a solution of XY in water. Draw an enthalpy diagram for the formation of this solution. What is the net AH for the formation of a solution of XY? i kJ mol-1

Some unknown compound reduces the freezing point of benzene from 5.53 to 4.80˚C. What is the molality of the benzene solution? The Kf for benzene is 5.12˚C/m.

Calculate the molality of a solution formed by adding 3.159 g of methanol (CH3OH) to 100.00 mL of water. The density of water is 0.9982 g/mL. DO not include units. The lattice energy for KF is 821 kJ/mol. The enthalpy of hydration for K+ is -336 kJ/mol and the enthalpy of hydration for F- is -431 kJ/mol. What is the enthalpy in kJ when 14.91 g of KF forms an aqueous solution? (Hint: start by finding the enthalpy of solution)

At 55.0 ∘C∘C, what is the vapor pressure of a solution prepared by dissolving 75.8 g of LiF in 247 g of water? The vapor pressure of water at 55.0 ∘C∘C is 118 mmHg. Assume complete dissociation of the solute.

You are analyzing 100 g of a solution that contains 12.5 g of the ionic compound KBr (MM = 119.0 g/mol) in water.  Here is some useful information:  KFP of water is 1.86 °C/m; KBP for water is 0.512 °C/m.  The density of the solution is 1.094 g/mL. Calculate the boiling point of this solution (bp of water is 100.0°C).   Calculate the osmotic pressure (in atm) of this solution at 25°C.

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

the separation of a mixture into pure substance 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the solution be saturated? Would you expect to see solid on the bottom of the container?

A small amount of acetonitrile (CH3CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) C B CH3 CN H₂O Use these sketches to answer the questions in the table below. soln The enthalpy of solution AH is negative when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage C to D? What force would oppose or favor the system moving from Stage C to D? Check all that apply. 0 absorbed released neither absorbed nor released none ionic bonding force covalent bonding force metal bonding force hydrogen-bonding force dipole force ion-dipole force dispersion force 0,0,... solution Ś

Camphor is a white solid that melts at 179.50°C. It has been used to determine the molecular weights of organic compounds because of its unusually large freezing-point-depression constant (39.7°C/m), which allows ordinary thermometers to be used. The organic compound is dissolved in camphor, and then the melting point of the solution is determined. If 1.08 g of an unknown compound is dissolved in 73.6 g camphor, the freezing point is found to be 177.09°C. What is the molecular weight of the unknown compound?

Which of the following phenomena is best described by Henry’s Law?a. Increasing temperature favors an endothermic process.b. The solubility of NaCl(s) in water increases with increasing temperature.c. The solubility of MgCl2(s) in water is unaffected by pressure.d. The vapor pressure of an aqueous solution of glucose, C6H12O6, is lower than the vapor pressure of pure water.e. The solubility of O2(g) in water increases with increasing pressure.