Chapter 8, Problem 8.134MP

Reaction of gaseous fluorine with compound X yields a single product Y, whose mass percent composition is 61.7% F and 38.3% Cl.

1. (a) What is a probable molecular formula for product Y, and what is a probable formula for X?
2. (b) Draw an electron-dot structure for Y, and predict the geometry around the central atom.
3. (c) Calculate ΔH° for the synthesis of Y using the following information:

  $\begin{array}{ll}2\text{ClF}(g)+{\text{O}}_2(g)\stackrel{}{\to }{\text{Cl}}_2\text{O}(g)+{\text{OF}}_2(g)\hfill & \Delta H°=+205.4\text{kJ}\hfill \\ 2{\text{ClF}}_3(l)+2{\text{O}}_2(g)\stackrel{}{\to }{\text{Cl}}_2\text{O}(g)+3{\text{OF}}_2(g)\hfill & \Delta H°=+532.8\text{kJ}\hfill \\ {\text{OF}}_2(g)\Delta H{°}_{\text{f}}=+24.5\text{kJ/mol}\hfill & \hfill \end{array}$

1. (d) How much heat in kilojoules is released or absorbed in the reaction of 25.0 g of X with a stoichiometric amount of F₂, assuming 87.5% yield for the reaction?