(Solved): 1. 2.  The equilibrium constant, \( K \), for the following reaction is \( 1.80 \times 10 ...

1. 2. 

The equilibrium constant, \( K \), for the following reaction is \( 1.80 \times 10^{-4} \) at \( 298 \mathrm{~K} \). \[ \mathrm{NH}_{4} \mathrm{HS}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g) \] \( 1.34 \times 10^{-2} \mathrm{M} \mathrm{H}_{2} \mathrm{~S} \). If the concentration of \( \mathrm{NH}_{3}(g) \) is suddenly increased to \( 1.97 \times 10^{-2} \mathrm{M} \), what will be the concentrations of the two gases once equilibrium has been reestablished? \[ \begin{array}{ll} {\left[\mathrm{NH}_{3}\right]=} & \mathrm{M} \\ {\left[\mathrm{H}_{2} \mathrm{~S}\right]=\mid} & \mathrm{M} \end{array} \] \[ \mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \] An equilibrium mixture of the three gases in a \( 1.00 \mathrm{~L} \) flask at \( 600 \mathrm{~K} \) contains \( 0.163 \mathrm{M} \mathrm{COCl}_{2}, 4.59 \times 10^{-2} \mathrm{M} \mathrm{CO}_{2} \) and \( 4.59 \times 10^{-2} \mathrm{M} \mathrm{Cl}_{2} \). What will be the concentrations of the three gases once equilibrium has been reestablished, if \( 3.64 \times 10^{-2} \mathrm{~mol} \) of \( \mathrm{CO}(\mathrm{g}) \) is added to the flask?