(Solved): CHEM 1225 worksheet (adapted from Dr. Greg Smith): Equilibrium expressions The equilibrium constan ...

CHEM 1225 worksheet (adapted from Dr. Greg Smith): Equilibrium expressions The equilibrium constant \( \mathrm{K} \) can be calculated only once the system has reached equilibrium. When the system is not at equilibrium, the ratio of products over reactions is referred to as the reaction quotient. This can be a useful number to gauge the current progress of the reaction: 1. The following partial pressures were recorded at \( 100^{\circ} \mathrm{C} \) for the below reaction: \[ \begin{array}{c} 2 \mathrm{NOBr}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\mathrm{~g}) \\ \mathrm{P}_{\mathrm{NOBr}}=0.10 \mathrm{~atm}, \mathrm{P}_{\mathrm{NO}}=0.10 \mathrm{~atm}, \mathrm{P}_{\mathrm{Br}_{2}}=0.10 \mathrm{~atm} \end{array} \] If \( K_{P}=60.6 \) at this temperature, calculate \( Q_{P} \) and predict which way the reaction will shift. 2. Consider the following reaction: \( 2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \mathrm{K}_{\mathrm{c}}=164 @ 298 \mathrm{~K} \) If a \( 2.25 \mathrm{~L} \) container currently has \( 0.055 \mathrm{~mol} \mathrm{NO}{ }_{2} \) and \( 0.082 \mathrm{~mol} \mathrm{~N}_{2} \mathrm{O}_{4} \), is the reaction at equilibrium? If not, which direction will it shift?