The equilibrium constant is \(2.4 \times 10^{3}\) at a certain temperature for the reaction

\[2 \mathrm{NO}(g) ightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)\]

For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift?

a. A 1.0-L flask contains \(0.024 \mathrm{~mol} \mathrm{NO}, 2.0 \mathrm{~mol} \mathrm{~N}_{2}\), and \(2.6 \mathrm{~mol} \mathrm{O}_{2}\).

b. A 2.0 -L flask contains \(0.032 \mathrm{~mol} \mathrm{NO}, 0.62 \mathrm{~mol} \mathrm{~N}_{2}\), and \(4.0 \mathrm{~mol} \mathrm{O}_{2}\).

c. A 3.0-L flask contains \(0.060 \mathrm{~mol} \mathrm{NO}, 2.4 \mathrm{~mol} \mathrm{~N}_{2}\), and \(1.7 \mathrm{~mol} \mathrm{O}_{2}\).

d. \(P_{\mathrm{NO}}=0.010 \mathrm{~atm}, P_{\mathrm{N}_{2}}=0.11 \mathrm{~atm}, P_{\mathrm{O}_{2}}=2.0 \mathrm{~atm}\)

e. \(P_{\mathrm{NO}}=0.0078 \mathrm{~atm}, P_{\mathrm{N}_{2}}=0.36 \mathrm{~atm}, P_{\mathrm{O}_{2}}=0.67 \mathrm{~atm}\)

f. \(P_{\mathrm{NO}}=0.0062 \mathrm{~atm}, P_{\mathrm{N}_{2}}=0.51 \mathrm{~atm}, P_{\mathrm{O}_{2}}=0.18 \mathrm{~atm}\)