Predict the ideal van’t Hoff factor (i) for KNO4.

For a given substance, which of the following phase transition is not endothermic?

An equilibrium that strongly favors products has ____________

Select the strongest intermolecular force in each of the following. 1) Br2 – [a] 2) CH4 – [b] 3) NH3 – [c] 4) BF3 – [d] 5) CH3Cl – [e]

A reaction mixture contains 0.0500 M NO, 0.0155 M Cl2, and 1.50 M NOCl for the reaction shown below: 2NO(g) + Cl2(g) ⇌ 2NOCl(g)              KC = 46000 at 400 K Show all your work and setup for credit. A) Calculate QC for the reaction. B) Is the reaction at equilibrium? C) If the reaction is not at equilibrium, will it proceed to form more reactants or more product?

How many grams of ethanol (C2H5OH) can be vaporized at its boiling point by 725 kJ of heat? (∆Hvap of ethanol is 38.56 kJ/mol, molar mass of ethanol = 46.068 g/mol) Show all your work and setup for credit.

Given the following four aqueous solutions (assume complete dissociation): Solution 1 0.36 m CH3CH2OH Solution 2 0.21 m CaF2 Solution 3 0.11 m NaBr Solution 4 0.32 m NH3   1) Which solution has the highest osmotic pressure? [a] 2) Which solution has the lowest boiling point? [b] 3) Which solution has the highest freezing point? [c] 4) Which solution has the lowest vapor pressure? [d]

Select the strongest intermolecular force in each of the following. 1) Cl2 – [a] 2) CCl4 – [b] 3) NF3 – [c] 4) BF3 – [d] 5) CH3OH – [e]

A 1.00 L of an aqueous solution contains 1.25 g of a nonionic solute. If the osmotic pressure of this solution at 25 oC is 0.3207 atm. 1) Calculate the molarity of the solution. [A] mol/L 2) Calculate the moles of the nonionic solute in the solution. [B] mol 3) Calcullate the molar mass of the nonionic solute. [C] g/mol

Select the substance with the weakest dispersion force from each of the following pairs. 1) BF3 or BCl3 [a] 2) CH3CH3 or CH3CH2CH2CH3 [b] 3) CCl4 or CF4 [c]