Help ASAP please

Question

At a temperature of 525 K the Keq = 0.041 for the following reaction:

PCl5(g) ⇄ PCl3(g) + Cl2(g)

At one point in time, measurements were taken and the following concentrations were measured:

[PCl5] = 0.77 mol/L, [PCl3] = 1.21 mol/L and [Cl2] = 0.49 mol/L

Is the system at equilibrium? If not, state which direction the reaction must shift to get to equilibrium

Answer 1

PCl5(g) <==> PCl3(g) + Cl2(g) ... Keq = 0.041

Calculate Q and compare it to Keq:

Q = [PCl3][Cl2] / [PCl5] = (1.21)(0.49) / (0.77) = 0.77

Since Q is greater than Keq, the system is NOT at equilibrium.

The system would have to produce less product and more reactant in order to the value of Q to approach the value of Keq, so the system would shift to the left (toward reactants).