A 1.00 L of an aqueous solution contains 1.25 g of a nonioni…

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 0.2668 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

A reaction mixture contains 0.0500 M NO, 0.0155 M Cl2, and 1…

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?

Given the following four aqueous solutions (assume complete…

Given the following four aqueous solutions (assume complete dissociation): Solution 1 0.30 m CH3OH Solution 2 0.32 m NH3 Solution 3 0.11 m MgSO4 Solution 4 0.18 m KBr   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]