Homework #4

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Page ID: 42483

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Due on Feb 10 (Wed)

Q1

What is the osmotic pressure, in atm, of an aqueous solution of 1.64 g of Ca(NO₃)₂ in water at 25 °C? The volume of the solution is 275 mL. (Hint: What is the van't Hoff factor assuming dilute solution behavior?)

Q2

What is the molar mass of a solution of 5.00 g of a compound in 25.00 g of carbon tetrachloride (bp 76.8 °C; Kb = 5.02 °C/m) that boils at 81.5 °C at 1 atm? (Hint: Compounds do NOT dissociate in nonpolar solvent such as CCl₄. What is the molality of the solution?)

Q3

The reaction below starts after adding 2.5 mol of NH₃,5.0 mol of N₂, and 7.5 mol of H₂ to a 5.00-L container. Calculate the reaction quotient and determine the direction in which the system will proceed to reach equilibrium.

\(\ce{2NH3}(g) \rightleftharpoons \ce{N2}(g)+\ce{3H2}(g) \hspace{20px} K_c=17\);

Q4

What is the molarity of H₂O after a mixture that contains [H₂O] = 1.00 M and [Cl₂O] = 1.00 M comes to equilibrium at 25 °C?

\(\ce{H2O}(g)+\ce{Cl2O}(g)⇌\ce{2HOCl}(g) \hspace{20px} K_c=0.10\)

(Hint: Let \(x\) be the decrease in [H₂O] to reach the equilibrium.Take the square root of \(K_c\) once you express \(K_c\) in terms of \(x\).)