In the 1980s, CFC-11 was one of the most heavily produced chlorofluorocarbons. The last step in its formation is

${\mathbf{CCI}}_{\mathbf{4}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{HF}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{}}\mathbf{}\mathbf{}\mathbf{\square }\mathbf{}\mathbf{}\mathbf{}{\mathbf{CFCI}}_{\mathbf{3}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{+}{\mathbf{HCI}}_{\mathbf{\left(}\mathbf{g}\mathbf{\right)}}$

If you start the reaction with equal concentrations of ${\mathbf{CCI}}_{\mathbf{4}}$and HF, you obtain

equal concentrations of ${\mathbf{CFCI}}_{\mathbf{3}}$and HCl at equilibrium. Are the final

concentrations of ${\mathbf{CFCI}}_{\mathbf{3}}$and HCl equal if you start with unequal

concentrations of${\mathbf{CCI}}_{\mathbf{4}}$ and HF? Explain.

CFC-11 is a strong greenhouse gas that depletes the ozone layer and is widely employed as a refrigerant in building chillers, a foam blowing agent in insulating foams, and a solvent. And CFC-11 emissions from eastern China showed that emissions from temperate western Asia and tropical Asia were growing significantly.

Rewrite the reaction as follows:

${\mathrm{CCI}}_{4\left(\mathrm{g}\right)}+{\mathrm{HF}}_{\left(\mathrm{g}\right)}\square {\mathrm{CFCI}}_{3\left(\mathrm{g}\right)}+{\mathrm{HCI}}_{\left(\mathrm{g}\right)}$

Assume the initial concentration${\mathrm{CCI}}_4$is y (M), and the initial concentration of HF is z

(M).

Assume x (M) of ${\mathrm{CCI}}_4$and x (M) of HF dissociate and the construct ICE table as

follows:

Equilibrium concentrations of ${\mathrm{CFCI}}_3$and HCl are equal for any initial concentrations

of ${\mathrm{CCI}}_4$and HF. This is due to equal stoichiometric coefficients for ${\mathrm{CFCI}}_3$and HCl in

the balanced equation.